Q1.
Thermodynamics is concerned with:
Q2.
A well stoppered thermos flask contains some ice cubes. This is an example of:
Q3.
Identify the intensive quantities from the following:
Q4.
Which of the following is an extensive property?
Q5.
For an adiabatic process which of the following relations is correct?
Q6.
In which of the following process work is independent of path?
Q7.
When a gas is compressed adiabatically and reversibly, the final temperature is:
Q8.
Which one is dependent on initial and final state?
Q9.
Out of boiling point (I), entropy (II), pH (III) and emf of a cell (IV), intensive properties are:
Q10.
The work done by a weightless piston in causing an expansion ΔV (at constant temperature), when the opposing pressure P is variable, is given by:
Q11.
The work done by 100 calorie of heat in isothermal expansion of ideal gas is:
Q12.
Temperature and volume are not:
Q13.
q = -w is not true for:
Q14.
The temperature of an ideal gas increase in an:
Q15.
Which statement is true for reversible process:
Q16.
Both q & w are _____ function:
Q17.
If work done by the system is 300 joule when 100 cal heat is supplied to it. The change in internal energy during the process is:
Q18.
A system has internal energy equal to E1, 450 J of heat is taken out of it and 600 J of work is done on it. The final energy of the system will be:
Q19.
The work done by a system is 8J when 40J heat is supplied to it. The change in internal energy of the system during the process:
Q20.
Internal energy change during a reversible isothermal expansion of an ideal gas is:
Q21.
Under which of the following conditions is the relation, ΔH = ΔE + PΔV valid for a system:
Q22.
The difference between heats of reaction at constant pressure and constant volume for the reaction 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) at 25°C in KJ is:
Q23.
For a gaseous reaction, A(g) + 3B(g) → 3C(g) + 3D(g), ΔE is 17 kCal at 27°C assuming R = 2 Cal K-1 mol-1, the value of ΔH for the above reaction is:
Q24.
Which of the following statements is correct for the reaction; 2SO2(g) + O2(g) → 2SO3(g) at constant temperature and pressure?
Q25.
For the reaction Ag2O(s) → 2Ag(s) + ½ O2(g), which one of the following is true:
Q26.
A mixture of 2 moles of carbon monoxide and one mole of oxygen in a closed vessel is ignited to get carbon dioxide. If ΔH is the enthalpy change and ΔE is the change in internal energy, then:
Q27.
For the gaseous reaction involving the complete combustion of isobutane:
Q28.
For the reversible isothermal expansion of one mole of an ideal gas at 300 K, from a volume of 10 dm3 to 20 dm3, ΔH is:
Q29.
For CaCO3(s) → CaO(s) + CO2(g) at 977°C, ΔH = 174 KJ/mol; then ΔE is:
Q30.
Heat of reaction for CO(g) + ½ O2(g) → CO2(g) at constant V is -67.71 K cal at 17°C. The heat of reaction at constant P at 17°C is:
Q31.
The enthalpy of vaporisation of water at 100°C is 40.63 kJ mol-1. The value ΔE for this process would be:
Q32.
For the system S(s) + O2(g) → SO2(g):
Q33.
For the reaction CO(g) + ½ O2(g) → CO2(g). Which one of these statement is correct at constant T and P?
Q34.
Which is true for the combustion of sucrose (C12H22O11) at 25°C:
Q35.
For which change ΔH ≠ ΔE:
Q36.
The heat of combustion of ethanol determined in a bomb calorimeter is -670.48 kCal mole-1 at 27°C. What is ΔH at 27°C for the reaction:
Q37.
The difference in ΔH and ΔE for the combustion of methane at 25°C would be:
Q38.
For which of the following reactions ΔH is less than ΔE:
Q39.
For a reaction 2X(s) + 2Y(s) → 2C(l) + D(g). The qp at 27°C is -28 kCal mol-1. The qV is _______ kCal mol-1:
Q40.
The work (in ergs) for a reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at 25°C is:
Q41.
Two moles of an ideal gas expand spontaneously into vacuum. The work is:
Q42.
One mole of a gas occupying 3 dm3 expands against a constant external pressure of 1 atm to a volume of 13 L. Find work is:
Q43.
For which reaction from the following, ΔS will be maximum?
Q44.
An adiabatic reversible process is one in which:
Q46.
\(\Delta S\) for the reaction: \(\text{MgCO}_3(s) \rightarrow \text{MgO}(s) + \text{CO}_2(g)\) will be:
Q47.
Change in entropy is negative for:
Q48.
In which reaction \(\Delta S\) is positive:
Q49.
When the egg is hard boiled, there is:
Q50.
If \(S^0\) for H2, Cl2 and HCl are 0.13, 0.22 and 0.19 kJ K-1 mol-1 respectively. The total change in standard entropy for the reaction \(\text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl}\) is:
Q51.
Which has the least entropy:
Q52.
When two gases are mixed the entropy:
Q53.
The enthalpy of vaporisation per mole of ethanol (B.pt. = 79.5°C and \(\Delta S = 109.8 \text{ JK}^{-1} \text{mol}^{-1}\)) is:
Q54.
If 900 J/g of heat is exchanged at boiling point of water, then what is increase in entropy?
Q55.
5 mole of an ideal gas expand reversibly from a volume of 8 dm3 to 80 dm3 at a temperature of 27°C. The change in entropy is:
Q56.
In a spontaneous irreversible process the total entropy of the system and surroundings:
Q57.
The total entropy change for a system & its surroundings increases if the process is:
Q58.
Calculate the entropy of Br2(g) in the reaction \(\text{H}_2(g) + \text{Br}_2(g) \rightarrow 2\text{HBr}(g)\), \(\Delta S^0 = 20.1 \text{ JK}^{-1}\) given, entropy of H2 and HBr is 130.6 and 198.5 J mol-1 K-1:
Q59.
In which of the following case entropy decreases:
Q60.
Which of the following quantity is not zero for element in standard state:
Q61.
Entropy of an adiabatic reversible process is:
Q62.
A gas is allowed to expand under reversible adiabatic conditions then:
Q63.
For a reaction at 25°C enthalpy change (\(\Delta H\)) and entropy change (\(\Delta S\)) are \(-11.7 \times 10^3 \text{ Jmol}^{-1}\) and \(-105 \text{ J mol}^{-1} \text{ K}^{-1}\) respectively. The reaction is:
Q64.
If \(\Delta H > 0\) and \(\Delta S > 0\), the reaction proceeds spontaneously when:
Q65.
The temperature at which the reaction \(\text{Ag}_2\text{O}(s) \rightarrow 2\text{Ag}(s) + \frac{1}{2}\text{O}_2(g)\) is at equilibrium is ........; Given \(\Delta H = 30.5 \text{ kJ mol}^{-1}\) and \(\Delta S = 0.066 \text{ kJK}^{-1} \text{mol}^{-1}\):
Q66.
Which of the following is true for the reaction \(\text{H}_2\text{O}(l) \rightleftharpoons \text{H}_2\text{O}(g)\) at 100°C and 1 atmosphere:
Q67.
For the reaction \(\text{A}(s) \rightarrow \text{B}(s) + \text{C}(g)\) the value of \(\Delta H = 30.56 \text{ kJ mol}^{-1}\) and \(\Delta S = 66 \text{ JK}^{-1} \text{mol}^{-1}\). The temperature at which the free energy change for the reaction will be zero is:
Q68.
For hypothetical reversible reaction \(\frac{1}{2}\text{A}_2(g) + \frac{3}{2}\text{B}_2(g) \rightarrow \text{AB}_3(g)\); \(\Delta H = -20 \text{ kJ}\) if standard entropies of A2, B2 and AB3 are 60, 40 and 50 JK-1 mole-1 respectively. The above reaction will be in equilibrium at:
Q69.
For the precipitation of AgCl by Ag+ ions and HCl:
Q70.
What is the sign of \(\Delta G\) for the process of ice melting at 1 atm, 283 K is?
Q71.
A reaction \(\text{A} + \text{B} \rightarrow \text{C} + \text{D} + q\) is found to have a positive entropy change, the reaction will be:
Q72.
Equilibrium constant of a reaction is related to:
Q73.
The Van't Hoff equation is:
Q74.
If \(\Delta G^0 > 0\) for a reaction then:
Q75.
If the equilibrium constant for a reaction is 10, then the value of \(\Delta G^0\) will be (R = 8 JK-1 mol-1, T = 300 K):
Q76.
The process of evaporation of a liquid is accompanied by:
Q77.
For the process, \(\text{CO}_2(s) \rightarrow \text{CO}_2(g)\):
Q78.
Which of the following provide exceptions to third law of thermodynamics:
Q79.
The Gibbs free energy change of a reaction at 27°C is -26 kCal and its entropy change is -60 Cal K-1. \(\Delta H\) for the reaction is:
Q80.
Which of the following reaction is expected never to be spontaneous:
Q81.
The formation of water from H2(g) and O2(g) is an exothermic process because:
Q82.
Which one of the following is not applicable for a thermochemical equation:
Q83.
The correct thermochemical equation is:
Q84.
The enthalpy changes of formation of the gaseous oxide of nitrogen (N2O and NO) are positive because of:
Q85.
\(\Delta H\) for transition of carbon from diamond form to graphite form is -453.5 Cal. This suggests that:
Q86.
Which of the following values of heat of formation indicates that the product is least stable:
Q87.
Heat of formation, \(\Delta H_f^0\), of an explosive compound like NCl3 is:
Q88.
According to the following reaction \(\text{C}(s) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}(g)\), \(\Delta H = -26.4 \text{ kCal}\):
Q89.
Which of the following represents an exothermic reaction:
Q90.
Consider the reaction \(3\text{O}_2 \rightarrow 2\text{O}_3\); \(\Delta H = +\text{Ve}\), from the reaction, we can say that:
Q91.
From the reaction P(White) → P(Red); \(\Delta H = -18.4 \text{ kJ}\), it follows that:
Q92.
In Kirchoff's equation which factor affects the heat of reaction:
Q93.
The enthalpy of a reaction at 273 K is -3.57 kJ. what will be the enthalpy of reaction at 373 K if \(\Delta C_p = 0\):
Q94.
For the reactions, (i) \(\text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(g) + x \text{ kJ}\) (ii) \(\text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(l) + y \text{ kJ}\) Which one of the following statement is correct:
Q95.
Since the enthalpy of formation of the elements in their standard states is taken to be zero. The heat of formation (\(\Delta H_f\)) of compounds:
Q96.
Reaction \(\text{H}_2(g) + \text{I}_2(s) \rightarrow 2\text{HI}\); \(\Delta H = 12.40 \text{ kCal}\). According to this, heat of formation of HI will be:
Q97.
Enthalpy of a compound is equal to its: (When it is formed from reference state of constituent elements)
Q98.
Which of the following equations represents standard heat of formation of CH4?
Q99.
The enthalpy of formation of ammonia is -46.0 kJ mol-1. The enthalpy change for the reaction \(2\text{NH}_3(g) \rightarrow \text{N}_2(g) + 3\text{H}_2(g)\) is:
Q100.
Given enthalpy of formation of CO2(g) and CaO(s) are -94.0 kJ and -152 kJ respectively and the enthalpy of the reaction: \(\text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g)\) is 42 kJ. The enthalpy of formation of CaCO3(s) is
Q101.
Given that standard enthalpy of formation of CH4, C2H4 and C3H8 are -17.9, 12.5, -24.8 kCal mol-1. The \(\Delta H\) for \(\text{CH}_4 + \text{C}_2\text{H}_4 \rightarrow \text{C}_3\text{H}_8\) is:
Q102.
The standard molar heat of formation of ethane, CO2 and water are respectively -21.1, -94.1 and -68.3 kCal. The standard molar heat of combustion of ethane will be
Q103.
The \(\Delta H_f^0\) for CO2(g), CO(g) and H2O(g) are -393.5, -110.5 and -241.8 kJ mol-1 respectively the standard enthalpy change (in kJ) for the reaction \(\text{CO}_2(g)+\text{H}_2(g) \rightarrow \text{CO}(g)+ \text{H}_2\text{O}(g)\) is:
Q104.
The enthalpies of combustion of carbon and carbon monoxide are -393.5 kJ and -283 kJ, respectively the enthalpy of formation of carbon monoxide is:
Q105.
The standard heat of formation of CS2(l) will be; given that the standard heat of combustion of carbon (s), sulphur(s) and CS2(l) are -393.3, -293.72 and -1108.76 kJ mol-1 respectively is
Q106.
The heat of combustion of CH4(g), C(s) and H2(g) at 25°C are -212.4 K Cal, -94.0 K Cal and -68.4 K Cal respectively, the heat of formation of CH4 will be:
Q107.
Standard enthalpy of formation is zero for:
Q108.
The standard heats of formation of NO2(g) and N2O4(g) are 8.0 and 2.0 kCal mol-1 respectively the heat of dimerization of NO2 in kCal is
Q109.
M is a metal that forms an oxide M2O \(\frac{1}{2}\text{M}_2\text{O} \rightarrow \text{M} + \frac{1}{4}\text{O}_2\) \(\Delta H = 120 \text{ kCal}\) When a sample of metal M reacts with one mole of oxygen what will be the \(\Delta H\) in that case
Q110.
According to equation, \(\text{C}_6\text{H}_6(l) + \frac{15}{2}\text{O}_2(g) \rightarrow 6\text{CO}_2(g) + 3\text{H}_2\text{O}(l)\); \(\Delta H = -3264.4 \text{ kJ mol}^{-1}\) the energy evolved when 7.8 g benzene is burnt in air will be:
Q111.
Heat of combustion of CH4, C2H6, C2H4 and C2H2 gases are -212.8, -373.0, -337.0 and -310.5 kCal respectively at the same temperature. The best fuel among these gases is:
Q112.
Given standard enthalpy of formation of CO (-110 kJ mol-1) and CO2(-394 kJ mol-1). The heat of combustion when one mole of graphite burns is
Q113.
The enthalpy of formation for C2H4(g), CO2(g) and H2O(l) at 25°C and 1 atm. pressure are 52, -394 and -286 kJ mole-1 respectively. The enthalpy of combustion of C2H4 will be:
Q114.
The combustion of one mole of benzene takes place at 298 K and 1 atm. After combustion, CO2(g) and H2O(l) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation, \(\Delta_f H^\circ\) of benzene. Standard enthalpies of formation of CO2(g) and H2O(l) are -393.5 kJ mol-1 and -285.83 kJ mol-1 respectively.
Q115.
The heat evolved during the combustion of 112 litre of water gas at STP (mixture of equal volume of H2 and CO) is: Given \(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(g)\); \(\Delta H = -241.8 \text{ kJ}\) and \(\text{CO}(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}_2(g)\); \(\Delta H = -283 \text{ kJ}\)
Q116.
A person requires 2870 kCal of energy to lead normal daily life. If heat of combustion of cane sugar is -1349 kCal mol-1, then his daily consumption of sugar is:
Q117.
The following are the heats of reactions: (i) \(\Delta H_f^0\) of H2O(l) = -68.3 kCal mol-1 (ii) \(\Delta H_{\text{comb}}\) of C2H2 = -337.2 kCal mol-1 (iii) \(\Delta H_{\text{comb}}\) of C2H4 = -363.7 kCal mol-1 Then heat change for the reaction \(\text{C}_2\text{H}_2 + \text{H}_2 \rightarrow \text{C}_2\text{H}_4\) is:
Q118.
The heat of combustion of a substance is:
Q119.
The value of \(\Delta H\) for the combustion of C(s) is -94.4 kCal. The heat of formation of CO2(g) is:
Q120.
In the combustion of 0.4 g of CH4, 0.25 kCal of heat is liberated. The heat of combustion of CH4 is:
Q121.
If \(\text{C}_6\text{H}_{12}\text{O}_6(s) + 9\text{O}_2(g) \rightarrow 6\text{CO}_2(g) + 6\text{H}_2\text{O}(g)\); \(\Delta H = -680 \text{ kCal}\). The weight of CO2(g) produced when 170 kCal of heat is evolved in the combustion of glucose is:
Q122.
Which of the following equations corresponds to the enthalpy of combustion at 298 K:
Q123.
Heat of formation of CO2 is -94.0 kCal. What would be the quantity of heat liberated, when 3 g of graphite is burnt in excess of oxygen:
Q124.
The amount of heat liberated when one mole of NH4OH reacts with one mole of HCl is:
Q125.
If \(\text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} + 13.7 \text{ kCal}\), then heat of complete neutralisation of one gram mole of H2SO4 with strong base will be:
Q126.
Heat of neutralisation of a strong dibasic acid in dilute solution by NaOH is nearly:
Q127.
The temperature of a 5 ml of strong acid increases by 5°C when 5 ml of a strong base is added to it. If 10 ml of each are mixed temperature should increase by:
Q128.
The heat of neutralization of HCl by NaOH is -55.9 kJ mol-1. If the heat of neutralization of HCN by NaOH is -12.1 kJ mol-1. The energy of dissociation of HCN is:
Q129.
If water is formed from H+ ions and OH- the heat exchange during the reaction:
Q130.
The change in the enthalpy of \(\text{NaOH} + \text{HCl} \rightarrow \text{NaCl} + \text{H}_2\text{O}\) is called:
Q131.
The heat of combustion of C2H4, C2H6 and H2 are -1409.5 kJ, -1558.3 kJ and -285.6 kJ. The heat of hydrogenation of ethene is:
Q132.
The enthalpy of combustion of cyclohexane, cyclohexene and H2 are respectively -3920, -3800 and -241 kJ mol-1. The heat of hydrogenation of cyclohexene is:
Q133.
Bond energy of a molecule:
Q134.
Among the following for which reaction heat of reaction represents bond energy of HCl:
Q135.
The bond energies of F2, Cl2, Br2 and I2 are 155.4, 243.6, 193.2 and 151.2 kJ mol-1 respectively. The strongest bond is:
Q136.
Energy required to dissociate 4g of gaseous hydrogen into free gaseous atoms is 208 kCal at 25°C. The bond energy of H-H bond will be:
Q137.
Heat evolved in the reaction \(\text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl}\) is 182 kJ. Bond energies of H-H and Cl-Cl are 430 and 242 kJ mol-1 respectively. The H-Cl bond energy is:
Q138.
The enthalpy change for the reaction \(\text{H}_2(g) + \text{C}_2\text{H}_4(g) \rightarrow \text{C}_2\text{H}_6(g)\) is........... . The bond energies are in kCal mol-1: H-H = 103, C-H = 99, C-C = 80 & C=C =145
Q139.
Bond dissociation enthalpies of H2(g) and N2(g) are 436.0 kJ mol-1 and 941.8 kJ mol-1 respectively and enthalpy of formation of NH3(g) is -46 kJ mol-1. What is enthalpy of atomization of NH3(g)?
Q140.
From the reactions: \(\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{CH}_4(g)\) \(\Delta H = -X\) kCal; \(\text{C}(g) + 4\text{H}(g) \rightarrow \text{CH}_4(g)\), \(\Delta H = -X_1\) kCal; \(\text{CH}_4(g) \rightarrow \text{CH}_3(g) + \text{H}(g)\) \(\Delta H = +Y\) kCal. Bond energy of C-H bond is:
Q141.
The enthalpy changes at 298 K in successive breaking of O-H bonds of water are \(\text{H}_2\text{O} \rightarrow \text{H}(g) + \text{OH}(g)\); \(\Delta H = 498 \text{ kJ mol}^{-1}\); \(\text{OH}(g) \rightarrow \text{H}(g) + \text{O}(g)\); \(\Delta H = 428 \text{ kJ mol}^{-1}\). The bond enthalpy of O-H bond is:
Q142.
If \(\Delta H_f^0\) of ICl(g), Cl(g), and I(g) is 17.57, 121.34 and 106.96 J mol-1 respectively. Then bond dissociation energy of ICl bond is:
Q143.
Heat of dissociation of benzene to elements is 5535 kJ mol-1. The bond enthalpies of C-C, C=C and C-H are 347.3, 615.0 and 416.2 kJ respectively. Magnitude of resonance energy of benzene is:
Q144.
The enthalpy change for the reaction \(2\text{C}(graphite) + 3\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\) is called:
Q145.
\(\text{Cl}_2(g) \rightarrow 2\text{Cl}(g)\), In this process value of \(\Delta H\) will be:
Q146.
The magnitude of heat of solution ..... on addition of solvent to solution:
Q147.
If \(\text{H}_2(g) \rightarrow 2\text{H}(g)\); \(\Delta H = 104 \text{ kCal}\), then heat of atomisation of hydrogen is:
Q148.
S(rhombic) + O2(g) → SO2(g); \(\Delta H = -297.5 \text{ kJ}\)
S(monoclinic) + O2(g) → SO2; \(\Delta H = -300 \text{ kJ}\)
The data can predict that:
Q149.
The heat of combustion of yellow phosphorous and red phosphorous are -9.91 kJ and -8.78 kJ respectively. The heat of transition of yellow phosphorous to red phosphorous is:
Q150.
\(2\text{CO}(g) + \text{O}_2(g) \rightarrow 2\text{CO}_2(g) + X \text{ kJ}\)
In the above equation X kJ refers to:
Q151.
\(\Delta H\) for the reaction, \(\text{I}(g) + \text{I}(g) \rightarrow \text{I}_2(g)\) will be:
Q152.
Given that: \(\text{A}(s) \xrightarrow{T K} \text{A}(l)\); \(\Delta H = x\), \(\text{A}(l) \xrightarrow{T K} \text{A}(g)\); \(\Delta H = y\). Calculate enthalpy of sublimation at 'T' K:
Q153.
The enthalpy change of a reaction does not depend on:
Q154.
From the thermochemical reactions, \(\text{C}(graphite) + \frac{1}{2}\text{O}_2 \rightarrow \text{CO}\); \(\Delta H = -110.5 \text{ kJ}\); \(\text{CO} + \frac{1}{2}\text{O}_2 \rightarrow \text{CO}_2\); \(\Delta H = -283.2 \text{ kJ}\). The heat of reaction of \(\text{C}(graphite) + \text{O}_2 \rightarrow \text{CO}_2\) is:
Q155.
If \(\text{H}_2 + \frac{1}{2}\text{O}_2 \rightarrow \text{H}_2\text{O}\); \(\Delta H = -68.39 \text{ kCal}\); \(\text{K} + \text{H}_2\text{O} + \text{water} \rightarrow \text{KOH}(aq) + \frac{1}{2}\text{H}_2\); \(\Delta H = -48.0 \text{ kCal}\); \(\text{KOH} + \text{water} \rightarrow \text{KOH}(aq)\) \(\Delta H = -14.0 \text{ kCal}\). The heat of formation of KOH is:
Q156.
Given: \(\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + 94.2 \text{ kCal}\); \(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l) + 68.3 \text{ kCal}\); \(\text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(l) + 210.8 \text{ kCal}\). The heat of formation of methane in Kcal will be:
Q157.
If, \(\text{H}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{HCl}(g)\); \(\Delta H^0 = -44 \text{ kCal}\); \(2\text{Na}(s) + 2\text{HCl}(g) \rightarrow 2\text{NaCl}(s) + \text{H}_2(g)\); \(\Delta H^0 = -152 \text{ kCal}\). Then, \(\text{Na}(s) + 0.5 \text{Cl}_2(g) \rightarrow \text{NaCl}(s)\); \(\Delta H^0 = ?\)
Q158.
(i) \(\text{S}(s) + \frac{3}{2}\text{O}_2(g) \rightarrow \text{SO}_3(g) + 2x \text{ kCal}\)
(ii) \(\text{SO}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{SO}_3(g) + y \text{ kCal}\)
Calculate the heat of formation of SO2:
Q159.
If \(\text{S} + \text{O}_2 \rightarrow \text{SO}_2\); \(\Delta H = -298.2 \text{ kJ}\); \(\text{SO}_2 + \frac{1}{2}\text{O}_2 \rightarrow \text{SO}_3\); \(\Delta H = -98.7 \text{ kJ}\); \(\text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4\); \(\Delta H = -130.2 \text{ kJ}\); \(\text{H}_2 + \frac{1}{2}\text{O}_2 \rightarrow \text{H}_2\text{O}\); \(\Delta H = -287.3 \text{ kJ}\). Then the enthalpy of formation of H2SO4 at 298 K is:
Q160.
Given that: \(\text{Zn} + \frac{1}{2}\text{O}_2 \rightarrow \text{ZnO} + 84000 \text{ Cal}\) ..................1; \(\text{Hg} + \frac{1}{2}\text{O}_2 \rightarrow \text{HgO} + 21700 \text{ Cal}\) ..................2. The heat of reaction (\(\Delta H\)) for, \(\text{Zn} + \text{HgO} \rightarrow \text{ZnO} + \text{Hg}\) is:
Q161.
Given that: \(2\text{C}(s) + 2\text{O}_2(g) \rightarrow 2\text{CO}_2(g)\) \(\Delta H = -787 \text{ kJ}\); \(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l)\) \(\Delta H = -286 \text{ kJ}\); \(\text{C}_2\text{H}_2(g) + \frac{5}{2}\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + \text{H}_2\text{O}(l)\) \(\Delta H = -1310 \text{ kJ}\). Heat of formation of acetylene is:
Q162.
The heat of reaction for \(\text{A} + \frac{1}{2}\text{O}_2 \rightarrow \text{AO}\) is -50 kCal and \(\text{AO} + \frac{1}{2}\text{O}_2 \rightarrow \text{AO}_2\) is 100 kCal. The heat of reaction for \(\text{A} + \text{O}_2 \rightarrow \text{AO}_2\) is:
Q163.
\(\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + 94.0 \text{ kCal}\); \(\text{CO}(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}_2(g)\), \(\Delta H = -67.7 \text{ kCal}\); from the above reactions find how much heat (kCal mole-1) would be produced in the following reaction: \(\text{C}(s) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}(g)\)
Q164.
The enthalpy of vapourisation of liquid water using the data: \(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l)\); \(\Delta H = -285.77 \text{ kJ mol}^{-1}\); \(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(g)\); \(\Delta H = -241.84 \text{ kJ mol}^{-1}\)
Q165.
\(\text{H}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{H}_2\text{O}(l)\); \(\Delta H_{298K} = -68.32 \text{ kCal}\). Heat of vapourisation of water at 1 atm and 25°C is 10.52 kCal. The standard heat of formation (in kCal) of 1 mole of water vapour at 25°C is:
Q166.
The heat of solution of anhydrous CuSO4 and CuSO4.5H2O are -15.89 and 2.80 kCal mol-1 respectively. What will be the heat of hydration of anhydrous CuSO4?
Q167.
Which of the following expressions is true: