2 moles of solid benzoic acid undergoes combustion at 300 K. C 6 H 5 COOH(s) +(15/2) O 2 (g) arrow 7 CO 2 (g) +3 H 2 O(l). The value of Δ H -Δ U value is

Question

2 moles of solid benzoic acid undergoes combustion at 300 K. C 6 H 5 COOH(s) +(15/2) O 2 (g) arrow 7 CO 2 (g) +3 H 2 O(l). The value of Δ H -Δ U value is (A) -1.247 kJ (B) -2.494 kJ (C) +2.494 kJ (D) +1.247 kJ

Tardigrade Admin · Accepted Answer

C 6 H 5 COOH(s) +(15/2) O 2 (g) arrow 7 CO 2 (g) +3 H 2 O(l) Δ H -Δ U =Δ n g RT =(-(1/2)(8.314) × 300/1000) =-1.247 kJ for two moles it is -2.494 kJ

Q. $2$ moles of solid benzoic acid undergoes combustion at $300 K$ .
$C_{6} H_{5} COO H (s) + \frac{15}{2} O_{2} (g) \to 7 C O_{2} (g) + 3 H_{2} O (l)$ .
The value of $Δ H - Δ U$ value is

$- 1.247 k J$

$- 2.494 k J$

$+ 2.494 k J$

$+ 1.247 k J$

$C_{6} H_{5} COO H (s) + \frac{15}{2} O_{2} (g) \to 7 C O_{2} (g) + 3 H_{2} O (l)$
$Δ H - Δ U = Δ n_{g} RT$
$= \frac{- \frac{1}{2} ( 8.314 ) \times 300}{1000}$
$= - 1.247 k J$ for two moles it is $- 2.494 k J$

Q. 2 moles of solid benzoic acid undergoes combustion at 300K. C6​H5​COOH(s)+215​O2​(g)→7CO2​(g)+3H2​O(l). The value of ΔH−ΔU value is

−1.247kJ

−2.494kJ

+2.494kJ

+1.247kJ