If for a certain reaction is 30 kJ mol–1 at 450 K, the value of (in JK–1 mol–1) for which the same reaction will be spontaneous at the same temperature is:
1. 70
2. –33
3. 33
4. –70
At standard conditions, if the change in the enthalpy for the following reaction is –109 kJ mol–1
H2(g)+Br2(g)2HBr(g) and the bond energy of H2 and Br2 is 435 kJ mol–1 and 192 kJ mol–1 respectively, what is the bond energy (in kJ mol–1) of HBr?
1. | 368 | 2. | 736 |
3. | 518 | 4. | 259 |
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. | \(C_{\mathrm{P}}-\mathrm{C}_{\mathrm{V}}=\mathrm{R}\) |
For irreversible expansion of an ideal gas under isothermal condition, the correct option is :
1.
2.
3.
4.
The correct option for free expansion of an ideal gas under adiabatic condition is:
1. and
2. and
3. and
4. and
For the reaction, 2Cl(g) Cl2(g), the correct option is:
1.
2.
3.
4.
Hydrolysis of sucrose is given by the following reaction
Sucrose + H2O Glucose + Fructose
If the equilibrium constant (Kc) is 21013 at 300 K, the value of at the same temperature will be:
1. 8.314 J mol–1 K–1300 Kln (21013)
2. 8.314 J mol–1 K–1300 Kln (31013)
3. –8.314 J mol–1 K–1300 Kln (41013)
4. –8.314 J mol–1 K–1300 Kln (21013)
1. | 2. | ||
3. | 4. |
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. | 1260 J | 2. | 2520 J |
3. | 5040 J | 4. | 0 J |