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OpenStudy (yerssonc):
for the reaction shown here 4PH3(g)<->6H2(g)+P4(g) the equilibrium concentrations were found to be [PH3] = .250 M [H2]= .510 M [P4]= .750 M what is the equilibrium constant for this reaction?
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OpenStudy (yerssonc):
Product/reactant = [H2]^ x [P4] / [P X H3]^4 = [.750] x [.510]^6 / [.250]^4 = 3.38
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