The difference between heat of reaction at constant pressure ( triangle H) and at constant volume (.ÎE.) for the reaction: C(s)+(1/2)O2 (g) arrow (CO)(g) is :- (Assume R=0.002KcalK- 1mol- 1 and temperature =TK )

Question

The difference between heat of reaction at constant pressure ( triangle H) and at constant volume (.ÎE.) for the reaction: C(s)+(1/2)O2 (g) arrow (CO)(g) is :- (Assume R=0.002KcalK- 1mol- 1 and temperature =TK ) (A) T cal (B) -T cal (C) -(T/2) cal (D) (T/2) cal

Tardigrade Admin · Accepted Answer

triangle H- triangle E= triangle ngRT =(1/2)× 0.002× TKcal =(T/2)cal

Q. The difference between heat of reaction at constant pressure $(△ H)$ and at constant volume $(Δ E)$ for the reaction: $C_{(s)} + \frac{1}{2} O_{2 (g)} \to (CO)_{(g)}$ is :-
(Assume $R = 0.002 Kc a l K^{- 1} m o l^{- 1}$ and temperature $= T K$ )

$T$ cal

$- T$ cal

$- \frac{T}{2}$ cal

$\frac{T}{2}$ cal

$△ H - △ E = △ n_{g} RT$
$= \frac{1}{2} \times 0.002 \times T Kc a l$
$= \frac{T}{2} c a l$

Q. The difference between heat of reaction at constant pressure (△H) and at constant volume (ΔE) for the reaction: C(s)​+21​O2(g)​→(CO)(g)​ is :- (Assume R=0.002KcalK−1mol−1 and temperature =TK )

T cal

−T cal

−2T​ cal

2T​ cal