Suppose a 500. mL flask is filled with 0.10 mol of CH4, 1.1 mol of IH2S and 1.8

Question

Suppose a 500. mL flask is filled with 0.10 mol of CH4, 1.1 mol of IH2S and 1.8 mol of IH2. This reaction becomes possible CH4(g)+2H,S(g)CS ()+4H2(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CS2 You can leave out the M symbol for molarity. H,S CS initial change equilibrium

Explanation / Answer

           CH4(g)    +   H2S(g)    ---->    CS2(g)   +   H2(g)

initial 0.1/0.5 = 0.2 M 1.1/0.5 = 0.55 M   0 M        1.8/0.5 = 0.9 M

change      -x               -x               +x           +x

equil     0.2-x M          0.55-x M            x M         0.9+x M

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