1. | 1260 J | 2. | 2520 J |
3. | 5040 J | 4. | 0 J |
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
1. | 2. | ||
3. | 4. |
1. | 120.9 kJ | 2. | 241.82 kJ |
3. | 18 kJ | 4. | 100 kJ |
For irreversible expansion of an ideal gas under isothermal condition, the correct option is :
1.
2.
3.
4.
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:
1. | 1.2 K | 2. | 2.4 K |
3. | 4.8 K | 4. | 6.6 K |
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 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