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Question

A certain reaction has value of Kp=0.0260 at 25oC and ΔrxnHo=32.4 kJ mol1. Calculate the value of Kp at 57oC.
antilog 0.55 = 3.55

A
0.1431
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B
0.0924
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C
0.2431
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D
0.0431
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Solution

The correct option is B 0.0924
Given, T1=25oC=25+273=298 K, T2=57oC=57+273=330 K, ΔrxnHo=32.4 kJmol1=32400 kJmol1, Kp1=0.0260
we know the van't Hoff equation is given by logKp2Kp1=H2.303R[T2T1T1T2]
putting the values we get,
logKp20.0260=324002.303×8.314[330298298×330]
logKp20.0260=3240019.147[3292380]
logKp20.0260=0.2198
Kp2=0.0924

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