Given that the equilibrium concentrations of [N2] = 0.035 M, [C2H2] = 0.057 M, and [HCN] = 6.8 x 10-4 M, find the value of the equilibrium constant expression for the reaction: N2(g) + C2H2(g) 2 HCN
a. 3.4 x 10-1
b. 2.9
c. 4300
d. 2.3 x 10-4
e. 6.8 x 10-1
1 comment April 27th, 2009
methyl ethanoate + water –> ethanol + ethanoic acid
The products were in solution forms, and yeh. I need some good varaibles/evaluation to say what could have gone wrong or what will effect the calculation of equilibrium constant. Kc was calculated as 0.18 which the actual value wa Kc=0.24
1 comment April 26th, 2009
The reaction shown below reaches equilibrium with the concentrations [H2O2] = 0.55, [H2O] = 0.75, [O2] = 0.15. What is the equilibrium constant for this reaction?
2H2O2(g) 2H2O(g) + O2(g)
2 comments April 26th, 2009
Suppose that the gas-phase reactions A->B and B->A are both elementary processes with rate constants of 3.8 x 10^-2 s^-1 and 3.l x 10^-1 s^-1, respectively.
A) What is the value of the equilibrium constant for the equilibrium A(g)-><-B(g)?
B) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B? Explain.
1 comment April 26th, 2009
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