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Given that ΔH°f(HCOOH,g) = -378.7kJ mol-1 and ΔH°f(HCOOH,l) = -425.0kJ mol-1. Calculate the vapor pressure of...

Given that ΔH°f(HCOOH,g) = -378.7kJ mol-1 and ΔH°f(HCOOH,l) = -425.0kJ mol-1.

Calculate the vapor pressure of formic acid in bar at 313.87 K, Using Clausius-clapeyron equation. Vapour pressure at 298.15K was calculated to be 0.0151bar from the previous question.

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Answer #1

HCOOH (4) → HCOOH (8) f HCOOR) 46.3 k3l mo P, Ξ O.OIS{ ba9a T2 ︵ 313.87ケ P, en P 433 314- L 298 151 313-g 7 O OIS↓ F 93S p 2

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