It is a chem equilibrium question, involving the ICE table.
The following reaction:
S2(g) + 2H2 (g) ←→ 2SH2(g)
takes place at high temperatures. If the initial amount of H2 and SH2 is 1.75 g and 1.95 g, respectively, and at equilibrium the amount of S2(g) is found to be 0.00188 atm, what is the value of the equilibrium constant? Please give your answer to three significant figures. Given: T = 1670 K and Reaction Volume = 0.500 L. (Hint: you will need to use the ideal gas law).
pv=nRT, ICE table
The Attempt at a Solution
What I did was find the the mols of H2 and SH2 since we are given n=m/M. So I have those 2 for "I" initial.
Then I found the equilibrium mols of S2, by plugging into the formula pv=nRt, solving for n=pv/Rt and I get 2.00E-5.
Essentially, I know K = [products]/[reactants]. But I only know the "I" of H2 and SH2, and I only know the "E" of S2.
Your help is greatly appreciated!