One mole of methanol when burnt in O₂ gives out 723 kJ mol^-1 of heat. If one mole of O₂ is used, what will be the amount of heat evolved?

1. 482 kJ
2. 241 kJ
3. 723 kJ               
4. 924 kJ

If the bond energies of H-H, Br-Br, and H-Br are 433, 192 and 364 kJ mol^-1 respectively, 

the $∆\mathrm{H}°$ for the reaction

H₂(g) + Br₂(g) $\to$2HBr(g) is

1.  -103 kJ               

2. -261 kJ

3. +103 kJ               

4. +261 kJ

For a given reaction, if ΔH = 35.5 kJ/mol and ΔS = 83.6 J/K·mol, at what temperature is the reaction spontaneous?
(Assume ΔH and ΔS remain constant with temperature.)

A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. The change in internal energy $∆$U of the gas in joules will be

(1) 1136.25 J

(2) - 500 J

(3) - 505 J

(4) + 515 J

For a sample of perfect gas when its pressure is changed isothermally from p_i to p_f, the entropy change is given by

(1) $∆$S = nRln(p_f/p_i)               

(2) $∆$S = nRln(p_i/p_f)

(3) $∆$S = nRTln(p_f/p_i)             

(4) $∆$S = RTln(p_f/p_i)

The correct thermodynamic conditions for the spontaneous reaction at all temperatures is

$\left(\mathrm{a}\right) ∆\mathrm{H}>0 \mathrm{and} ∆\mathrm{S}<0$
$\left(\mathrm{b}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}>0$
$\left(\mathrm{c}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}<0$
$\left(\mathrm{d}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}=0$

The heat of combustion of carbon to CO₂ is -393.5 kJ/mol. The heat released upon the

formation of 35.2 g of CO₂ from carbon and oxygen gas is

1. -315 kJ               

2. +315 kJ             

3. -630 kJ                 

4. -3.15 kJ

For the reaction, X₂O₄(l) $\to$2XO₂(g)

$∆$U = 2.1 kcal, $∆$S = 20 cal K^-1 at 300 K. Hence, $∆$G is

1. 2.7 kcal

2. -2.7 kcal

3. 9.3 kcal

4. -9.3 kcal

The standard enthalpy of vaporisation $∆$_vapH$°$ for water at 100$°$C is 40.66 kJ mol^-1. The

internal energy of vaporisation of water at 100$°$C (in kJ mol^-1) is- 

(Assume water vapour to behave like an ideal gas)

1. +37.56                   

2. -43.76

3. +43.76                   

4. +40.66

If the enthalpy change for the transition of liquid water to steam is 30 kJ mol^-1 at 27°C,

the entropy change for the process would be

1. 1.0 J mol^-1 K^-1

2. 0.1 J mol^-1K^-1

3. 100 J mol^-1K^-1

4. 10 J mol^-1K^-1