for the following reaction is:
1. | -731 J | 2. | -1317 J |
3. | -501 J | 4. | +731 J |
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 |
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
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)
If the bond energies of H–H, Br – Br, and H –Br are 433, 192, and 364 kJ mol–1 respectively, the ∆Hº for the reaction H2(g) + Br2(g) → 2HBr(g) will be:
1. +103 kJ
2. +261kJ
3. –103 kJ
4. –261 kJ