Calculate the partial pressure (in atm) of S2 at equilibrium when 1.47 atm of H2

Question

Calculate the partial pressure (in atm) of S2 at equilibrium when 1.47 atm of H2S dissociates at 600 K according to the following chemical equilbrium 2H2S(g) 2H2(g) + S2(g) Kp = 4.55 Times 10-11 If the 5% approximation is valid, use the assumption to compute the partial pressure. Report your answer to three significant figures in scientific notation Without doing any calculations, predict the sign of Delta Ssys for each of the following processes: Answer the following questions using the chemical reaction and thermochemical information given below: 2HBr(g) 1Br2(g) + H2(g) Determine Delta G degree rx (in kJ) for this reaction at 10576.25 K. Assume Delta H degree f and S degree do not vary as a function of temperature. Report your answer to two decimal Determine the equilibrium constant for this reaction. Report your answer to three significant figures in scientific notation.

Explanation / Answer

P^3/(1.47)^2 = 4.55*10^-11

solving, P = 4.61*10^-4 atm

delta S system:

1. -ve

2. +ve

3. -ve

4. -ve

delta G = delta H - T delta S

= 67.19*1000 - (10576.25*177.48)

= - 1809.88 KJ

equilibrium constant = exp (-delta G/ RT)= 8.69*10^8

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