You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Bond Order and Enthalpy

SO2g+12O2g→ S...

Question

$S O_{2} (g) + \frac{1}{2} O_{2} (g) \to S O_{3} (g)$
is exothermic reaction by change in internal energy $97030 J$ at $298 K$ and 1 atm at constant volume measured in a bomb calorimeter. The value of $Δ H$ is

-100 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

-98.2 kJ

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

-102.4 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

-95.8 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B -98.2 kJ
For Exothermic, $(Change in internal energy) Δ U = - 97030 J$

$(Change in Enthaply) Δ H = Δ U + Δ n R T$

$\Rightarrow S O_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ S O_{2} (g)$

$\Rightarrow Δ n = - 0.5$

$\Rightarrow Δ H = - 97030 + (- 0.5 \times 8.314 \times 298) = - 98268.78 J$

$\Rightarrow Δ H = - 98.2 k J$
Hence correct option is (b)

Suggest Corrections

Similar questions

Chemical reaction is invariably associated with the transfer of energy either in the form of heat or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called Calorimeter. Heat change in the process is calculated as :

q = m s Δ T

........

s = s p e c i f i c h e a t

= c Δ T

.......

c = h e a t c a p a c i t y

Heat of reaction at constant volume is measured using bomb Calorimeter.

q_{V} = Δ U =

internal energy change
Heat of reaction at constant pressure is measured using bomb Calorimeter.

q_{P} = Δ H

q_{P} = q_{V} + P Δ V

Δ H = Δ U + Δ n R T

The heat capacity of a bomb calorimeter is

500 J K^{- 1}

. When

0.1 g

of Methane was burnt in this calorimeter, the temperature rose by

2^{\circ} C

. The value of

Δ U

per mole will be :

Q. For the reaction

C H_{3} C O O H (l) + 2 O_{2} (g) ⇌ 2 C O_{2} (g) + 2 H_{2} (g) + 2 H_{2} O (l)

25^{\circ} C

and 1 atm pressure,

Δ H = - 874 K J

Then the change in internal energy (

Δ

E) is

The reaction of cyanamide, $N H_{2} C N_{(s)}$ , with dioxygen was carried out in a bomb calorimeter, and $Δ U$ was found to be $- 742.7 k J m o l^{- 1}$ at 298 K. calculate enthalpy change for the reaction at 298 K.
$N H_{2} C N_{(g)} + \frac{3}{2} O_{2 (g)} \to N_{2 (g)} + C O_{2 (g)} + H_{2} O_{(l)}$

Q. The heat of combustion of gaseous methane

({C H}_{4})

at constant volume is measured in a bomb calorimeter at 298 K and is found to be

- 885.4 k J {m o l}^{- 1}

. Find the value of enthalpy change.

In a constant volume calorimeter 5g of a gas with molecular weight 40 was burnt in excess of oxygen at 298K. The temperature of the calorimeter was found to increase from 298K to 298.75K due to combustion process. Given that the heat capacity of the calorimeter is 2.5kJK^-1 , the numerical value for the change in internal energy of combustion of the gas in kJ /mol is?

Join BYJU'S Learning Program

SO2(g)+12O2(g)→SO3(g) is exothermic reaction by change in internal energy 97030J at 298K and 1 atm at constant volume measured in a bomb calorimeter. The value of ΔH is

The correct option is B -98.2 kJFor Exothermic, (Change in internal energy)ΔU=−97030 J (Change in Enthaply)ΔH=ΔU+ΔnRT ⇒SO2(g)+12O2(g)⟶SO2(g) ⇒Δn=−0.5 ⇒ΔH=−97030+(−0.5×8.314×298)=−98268.78 J ⇒ΔH=−98.2 kJ Hence correct option is (b)

$S O_{2} (g) + \frac{1}{2} O_{2} (g) \to S O_{3} (g)$
is exothermic reaction by change in internal energy $97030 J$ at $298 K$ and 1 atm at constant volume measured in a bomb calorimeter. The value of $Δ H$ is