Consider the following reaction:
\(\mathrm{2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \Delta_rH^\circ = -483.64 kJ. }\)
What is the enthalpy change for the decomposition of one mole of water?
1. 120.9 kJ
2. 241.82 kJ
3. 18 kJ
4. 100 kJ

The work done when 1 mole of gas expands reversibly and isothermally from a pressure of 5 atm to 1 atm at 300 K is: ​
(Given log 5 = 0.6989 and R = 8.314 J K^-1 mol^-1)
1. zero J
2. 150 J
3. +4014.6 J
4. -4014.6 J

For irreversible expansion of an ideal gas under isothermal condition, the correct option is :

1. $∆\mathrm{U}=0, ∆{\mathrm{S}}_{\mathrm{total}}\ne 0$

2. $∆\mathrm{U}\ne 0, ∆{\mathrm{S}}_{\mathrm{total}}=0$

3. $∆\mathrm{U}=0, ∆{\mathrm{S}}_{\mathrm{total}}=0$

4. $∆\mathrm{U}\ne 0, ∆{\mathrm{S}}_{\mathrm{total}}\ne 0$

Which of the following options correctly represents the relationship between \(C_p \text { and } C_V\) for one mole of an ideal gas?

1. \(C_P=R C_V \)
2. \(C_V=RC_P \)
3. \(C_P+C_V=R \)
4. \(C_{\mathrm{P}}-\mathrm{C}_{\mathrm{V}}=\mathrm{R}\)

The molar heat capacity of water at constant pressure, C, is 75 JK^–1 mol^–1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of the water is:

For which one of the following equations is $∆\mathrm{H}{°}_{\mathrm{react}}$ equal to $∆\mathrm{H}{°}_{\mathrm{f}}$ for the product:

1. N₂(g) + O₃(g) → N₂O₃(g)

2. CH₄(g) + 2Cl₂(g) → CH₂Cl₂(l) + 2HCl(g)

3. Xe(g) + 2F₂(g) → XeF₄(g)

4. 2CO(g) + O₂(g) → 2CO₂(g)

The formation of a solution from two components can be considered as:

The solution so formed will be ideal if:
1. ∆H_Soln = ∆H₁ + ∆H₂ + ∆H₃

2. ∆H_Soln = ∆H₁ + ∆H₂ – ∆H₃

3. ∆H_Soln = ∆H₁ – ∆H₂ – ∆H₃

4. ∆H_Soln = ∆H₃ – ∆H₁ – ∆H₂