Given below are two statements:

Assertion (A):	The standard heat of combustion of a hydrocarbon compound is an intensive property.
Reason (R):	The standard heat of combustion is considered an intensive property because the amount of the substance is defined as 1 mole.

 

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

The temperature of 5 ml of a strong acid increases by $5^{\circ }$ when 5 ml of a strong base is added to it. If 10 ml of each is mixed, temperature should increase by-

1. $5^{\circ }$

2. ${10}^{\circ }$

3. ${15}^{\circ }$

4. cannot be known

The heat of neutralisation of HCl by NaOH is -55.9 kJ/mole. If the heat of neutralisation of HCN by NaOH is -12.1 kJ/mole, then energy of dissociation of HCN is-

1. -43.8 kJ

2. 43.8 kJ

3. 68 kJ

4. -68 kJ

For a reaction at equilibrium-

1. $∆G=∆G^{\circ }=0$

2. $∆G=0<mspace\; width="1em"></mspace>but<mspace\; width="1em"></mspace>not<mspace\; width="1em"></mspace>∆G^{\circ }$

3. $∆G^{\circ }=0<mspace\; width="1em"></mspace>but<mspace\; width="1em"></mspace>not<mspace\; width="1em"></mspace>∆G$

4. $∆G=∆G^{\circ }\ne 0$

Using only the following data:

(I) $F{e}_2{O}_3\left(s\right)+3CO\left(g\right)\rightleftharpoons 2Fe\left(s\right)+3C{O}_2\left(g\right);$
$∆H^{\circ }=-26.8<mspace\; width="1em"></mspace>kJ$

(II) $$\begin{gathered} Fe\left(s\right)+C{O}_2\left(g\right)\rightleftharpoons FeO\left(s\right)+CO\left(g\right); \\ ∆H^{\circ }=+16.5<mspace\; width="1em"></mspace>kJ \end{gathered}$$

the $∆H^{\circ }$ value, in kilojoules, for the reaction

$F{e}_2{O}_3\left(s\right)+CO\left(g\right)\to 2FeO\left(s\right)+C{O}_2\left(g\right)$ is calculated to be:

1. -43.3

2. -10.3

3. +6.2

4. +10.3

82 litres of carbon dioxide are produced at a pressure of 1 atm by the action of acid on a metal carbonate. The work done at room temp by the gas (in calories) in pushing back the atmosphere is 

1. 1000

2. 820

3. 1640

4. 2200

Among the following, the reaction for which $∆H=∆E$ is-

1. $PC{l}_5\left(g\right)\to PC{l}_3\left(g\right)+C{l}_2\left(g\right)$

2. $H_2\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)$

3. $C_2{H}_{5}OH\left(l\right)+3O_2\left(g\right)\to 2C{O}_2\left(g\right)+3H_{2}O\left(l\right)$

4. $C_2{H}_4\left(g\right)+H_2\left(g\right)\to C_2{H}_6\left(g\right)$

For which change $∆H\ne ∆E$

1. $H_2+I_2\rightleftharpoons 2HI$

2. $HCl+NaOH\to NaCl+H_{2}O$

3. $C\left(s\right)+O_2\left(g\right)\rightleftharpoons C{O}_2\left(g\right)$

4. $N_2+3H_2\to 2N{H}_3$

Enthalpy change when 1.00 g water is frozen at $0^{\circ }C,$ is :

$\left(∆H_{fus}=1.435<mspace\; width="1em"></mspace>kcal<mspace\; width="1em"></mspace>mo{l}^{-1}\right)$

1. 0.0797 kcal

2. -0.0797 kcal

3. 1.435 kcal

4. -1.435 kcal

One mole of hydrogen gas at ${25}^{\circ }C$ and 1 atm pressure is heated at constant pressure until its volume has doubled. Given that $C_v$ for hydrogen is 3.0 cal deg^-1 mol^-1, the $∆H<mspace\; width="1em"></mspace>$and $∆E$ for this process are-

1. $∆H<mspace\; width="1em"></mspace>$= 1490 cal and $∆E$ = 894 cal

2. $∆H<mspace\; width="1em"></mspace>$= $∆E$= 1490 cal

3. $∆H<mspace\; width="1em"></mspace>$= 894 cal and $∆E$= 1490 cal

4. $∆H<mspace\; width="1em"></mspace>$= $∆E$= 894 cal