For the following reaction: LiBr(s) + H2(g) LiH(s) + HBr(g) Kp = 7.06 Times 10-3

Question

For the following reaction: LiBr(s) + H2(g) LiH(s) + HBr(g) Kp = 7.06 Times 10-3 What is the value of Kp for the reverse reaction? Report your answer to three significant figures in scientific notation. What is the value of Kp if the stoichiometric coefficients for the forward reaction are halved? Report your answer to three significant figures in scientific notation. Given the following process, will it be spontaneous only at high temperatures, low temperatures, all temperatures, or never? 2C7H14(I) + 21O2(g) rightarrow 14CO2(g) + 14H2O(I) Delta Hrx= -9315.36 kJ Delta Srx= -1004 J/K

Explanation / Answer

1.kp= -7.6*10-3

2.raise to the powr value n times

3.at lower temperature spontaneous

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