For the reaction, $2C{}^{}\to C{}^{}$, the value of ∆H and ∆S  are respectively -

1. $∆\mathrm{H}=0$ $,$ $∆\mathrm{S}=-\mathrm{ve}$

2. $∆\mathrm{H}=0$ $,$ $∆\mathrm{S}=0$

3. $∆\mathrm{H}=$ $-\mathrm{ve}$ $,$ $∆\mathrm{S}$ $=$ $-\mathrm{ve}$

4. $∆\mathrm{H}=$ $+\mathrm{ve}$ $,$ $∆\mathrm{S}=$ $+\mathrm{ve}$

The enthalpy of combustion of carbon to CO₂ is –393.5 kJ mol^-1. The amount of heat released upon formation of 35.2 g of CO₂ from carbon and dioxygen gas would be-

1. -393.5 kJ mol^-1

2. -314.8 kJ mol^-1

3. +314.8 kJ mol^-1

4. -320.5 kJ mol^-1

 For the reaction A + B → C + D + q (kJ/mol), entropy change is positive. The reaction will be

1. Possible only at high temperature

2. Possible only at low temperature

3. Not possible at any temperature

4. Possible at any temperature

The enthalpy of combustion of methane, graphite, and dihydrogen at 298 K are,

–890.3 kJ mol^-1 , –393.5 kJ mol^-1, and –285.8 kJ mol^-1 respectively.

The enthalpy of formation of CH₄(g) is-

1.  –74.8 kJ mol^-1

2.  –52.27 kJ mol^-1

3.  +74.8 kJ mol^-1

4.  +52.26 kJ mol^-1

Match the following process with entropy change

Codes

Match the following parameters with a description for spontaneity.

Codes

Thermodynamics is not concerned about-

1. Energy changes involved in a chemical reaction

2. The extent to which a chemical reaction proceeds

3. The rate at which a reaction proceeds

4. The feasibility of a chemical reaction