For which one of the following equations is equal to 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 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:
1. | 1.2 K | 2. | 2.4 K |
3. | 4.8 K | 4. | 6.6 K |
The formation of a solution from two components can be considered as:
(i) | Pure solvent → separated solvent molecules, ∆H1 |
(ii) | Pure solute → separated solute molecules, ∆H2 |
(iii) | Separated solvent and solute molecules → solution, ∆H3 |
The solution so formed will be ideal if:
1. ∆HSoln = ∆H1 + ∆H2 + ∆H3
2. ∆HSoln = ∆H1 + ∆H2 – ∆H3
3. ∆HSoln = ∆H1 – ∆H2 – ∆H3
4. ∆HSoln = ∆H3 – ∆H1 – ∆H2
What is the entropy change (in JK–1 mol–1) when one mole of ice is converted into water at 0 ºC? (The enthalpy change for the conversion of ice to liquid water is 6.0 KJ mol–1 at 0 ºC)
1. | 20.13 | 2. | 2.013 |
3. | 2.198 | 4. | 21.98 |
The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm–3, respectively. If the standard free energy difference (∆Gº) is equal to 1895 J mol–1, the pressure at which graphite will be transformed into diamond at 298 K is:
1. 11.08
2.
3.
4. 11.08
For the reaction:
\(C_{3} H_{8} \left(\right. g \left.\right) + 5 O_{2} \left(\right. g \left.\right) \rightarrow 3 CO_{2} \left(\right. g \left.\right) + 4 H_{2} O \left(\right. l \left.\right)\) at constant temperature, ∆H – ∆E is:
1. | + RT | 2. | – 3RT |
3. | + 3RT | 4. | – RT |
Enthalpy of is negative. If the enthalpy of combustion of are x and y respectively, then which relation is correct:
1. | x > y | 2. | x < y |
3. | x = y | 4. | x ≥ y |
When 1 mol gas is heated at constant volume, the temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. The correct statement among the following is:
1. q = w = 500 J, ∆U = 0
2. q = ∆U = 500 J, w = 0
3. q = w = 500 J, ∆U = 0
4. ∆U = 0, q = w = – 500 J
For the given reaction
, the heat of formations of are -188 kJ/mol & -286 KJ/mol respectively. The change in the enthalpy of the reaction will be:
1. – 196 kJ/mol
2. + 196 kJ/mol
3. + 948 kJ/mol
4. – 948 kJ/mol
Heat of combustion ∆Hº for C(s), H2(g) and CH4(g) are – 94, – 68 and – 213 Kcal/mol. ∆Hº for C(s) + 2H2(g) → CH4 (g) is:
1. | – 17 Kcal | 2. | – 111 Kcal |
3. | – 170 Kcal | 4. | – 85 Kcal |