The difference between heats of reaction at constant pressure and at constant volume for the reaction
$2 C_{2} H_{6 (l)} + {7 O}_{2} (g) \to 4 {C O}_{2} (g) + 6 H_{2} O (l) a t 25^{0} C$ in kJ is:

-7.43 kJ

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

+3.72 kJ

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

-3.72 kJ

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

+7.43 kJ

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

Open in App

Solution

The correct option is A -7.43 kJ
$Δ H = Δ U + Δ_{n_{g a s}} R T$

$\Rightarrow Δ H - Δ U = Δ_{n_{g a s}} R T$

$Δ_{n_{g a s}} R T = 12 - 15 = (- 3)$

$∴ Δ_{n_{g a s}} R T = \frac{- 3 \times 8.314 \times 298}{1000} k J$

$\approx - 7.43 k J$

Suggest Corrections

Similar questions

Q. The difference between heats of reaction at constant pressure and at constant volume for the reaction

2 C_{6} H_{6} (l) + 15 O_{2} (g) \to 12 C O_{2} (g) + 6 H_{2} O (l) a t 25^{\circ} C

at in kJ is

The difference between heats of Reaction at constant pressure and constant volume for the Reaction $2 C_{6} H_{6} + 15 O_{2} \to 12 C O_{2} + 6 H_{2} O$ at $25^{\circ} C$ . in $k J$ is

Q. The difference between heat of reaction at constant pressure and constant volume for the reaction

2 C_{6} H_{6 (l)} + 15 O_{2 (g)} \to 12 C O_{2 (g)} + 6 H_{2} O_{(l)}

25^{\circ} C

in KJ is

Q. The difference between heat of reaction at constant pressure and constant volume for the reaction given below at

25^{\circ} C

k J

is :

A (g) + 3 B (g) \to C (g)

Q. The difference between the heats of a reaction at constant pressure and volume for the reaction

2 C_{6} H_{6} (l) + 15 O_{2} (g) \to 12 C O_{2} (g) + 6 H_{2} O (l)

at 25°C in kJ is:

Join BYJU'S Learning Program

The difference between heats of reaction at constant pressure and at constant volume for the reaction2C2H6(l)+7O2(g)→4CO2(g)+6H2O(l) at 250C in kJ is:

The correct option is A -7.43 kJΔH=ΔU+ΔngasRT ⇒ΔH−ΔU=ΔngasRT ΔngasRT=12−15=(−3) ∴ΔngasRT=−3×8.314×2981000kJ ≈−7.43kJ

The difference between heats of reaction at constant pressure and at constant volume for the reaction
$2 C_{2} H_{6 (l)} + {7 O}_{2} (g) \to 4 {C O}_{2} (g) + 6 H_{2} O (l) a t 25^{0} C$ in kJ is:

The correct option is A -7.43 kJ
$Δ H = Δ U + Δ_{n_{g a s}} R T$

$\Rightarrow Δ H - Δ U = Δ_{n_{g a s}} R T$

$Δ_{n_{g a s}} R T = 12 - 15 = (- 3)$

$∴ Δ_{n_{g a s}} R T = \frac{- 3 \times 8.314 \times 298}{1000} k J$

$\approx - 7.43 k J$