Which of the following is not a state function?

1.	ΔS	2.	ΔG
3.	ΔH	4.	ΔQ

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 liters to 20 liters at 25°C is -

1. $-2.303\times 298\times 0.082$ $\log$ $2$

2. $-298\times {10}^7\times 8.31\times 2.303$ $\log$ $2$

3. $2.303\times 298\times 0.082$ $\log$ $0.5$

4. $-8.31\times {10}^7\times 298-2.303$ $\log$ $0.5$

Consider the given reaction:
\(C H_{3} C O O H \left(\right. l \left.\right)+ 2 O_{2} \left(\right. g \left.\right) \rightleftharpoons 2 C O_{2} \left(\right. g \left.\right)+ 2 H_{2} O \left(\right. l \left.\right)\)
At 25°C and 1 atm. pressure, ΔH = –874 kJ. The change in internal energy (ΔE) is:

1. – 874 kJ
2. – 971.53 kJ
3. + 971.53 kJ
4. + 874 kJ

The occurrence of a reaction is impossible if:

1. ΔH is +ve ; ΔS is also + ve but ΔH < TΔS

2. ΔH is – ve ; ΔS is also – ve but ΔH > TΔS

3. ΔH is – ve ; ΔS is + ve

4. ΔH is + ve ; ΔS is – ve

The unit of entropy is -

1. J mol^–1

2. JK mol^–1

3. J mol^–1 K^–1

4. J^–1 K^–1 mol^–1

Combustion of glucose takes place according to the equation,

${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6+6{\mathrm{O}}_2\to 6{\mathrm{CO}}_2+6{\mathrm{H}}_2\mathrm{O}$, $∆<mspace\; width="1em"></mspace>H<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-72<mspace\; width="1em"></mspace>K<mspace\; width="1em"></mspace>cal$

Energy required for the production of 1.6 g of glucose is -

(Molecular mass of glucose = 180 g)

1. 0.064 kcal

2. 0.64 kcal

3. 6.4 kcal

4. 64 kcal

When a gas undergoes adiabatic expansion, it gets cooled due to -

1. Loss of energy

2. Fall in pressure

3. Decrease in velocity

4. Increase in energy with work done

A Beckmann thermometer is used to measure -

1. High temperature

2. Low temperature

3. Normal temperature

4. All temperatures

$The<mspace\; width="1em"></mspace>factor<mspace\; width="1em"></mspace>{\left(\frac{\partial Q}{\partial T}\right)}_P<mspace\; width="1em"></mspace>-<mspace\; width="1em"></mspace>{\left(\frac{\partial Q}{\partial T}\right)}_V<mspace\; width="1em"></mspace>is<mspace\; width="1em"></mspace>equal<mspace\; width="1em"></mspace>to:$

1. $\gamma$

2. R

3. $\frac{R}{M}$

4. $∆\mathrm{nRT}$

Which plot represents an exothermic reaction?

1.		2.
3.		4.