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

C 6 H 5 COOH s + 15 2 O 2 g → 7 CO 2 g + 3 H 2 O l Δ H – Δ U = Δ n g R T = – 1 2 ( 8.314 ) × 300 1000 = − 1.247 kJ for two moles it is − 2.494 kJ

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ChemistryThermochemistryAdiabatic Process/PolytropicMedium2 minPYQ_2020

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

Options:

Answer:

Solution:

$C_{6} H_{5} COOH (s) + \frac{15}{2} O_{2} (g) \to 7 {CO}_{2} (g) + 3 H_{2} O (l)$
$Δ H - Δ U = Δ n_{g} R T$
$= \frac{(- \frac{1}{2}) (8.314) \times 300}{1000}$
$= - 1.247 kJ$ for two moles it is $- 2.494 kJ$

Stream:NTA_ABHYASSubject:ChemistryTopic:ThermochemistrySubtopic:Adiabatic Process/Polytropic

⏱ 2mℹ️ Source: PYQ_2020

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