# College Chemistry

posted by .

The initial concentration for the compounds involved in the reaction shown were determined to be [CH4(g)] = 0.6616 mol/L, [H2O(g)] = 0.8127 mol/L, [CO(g)] = 0.9566 mol/L, [H2(g)] = 0.7688 mol/L. Calculate the value of the equilibrium constant (Kc) at 1200 K if the equilibrium concentration of CO(g) was 0.8900 mol/L.

CH4(g)+H2O(g) = CO(g)+3H2(g)

• College Chemistry -

......CH4 + H2O ==> CO + 3H2
I..0.6616.0.8127..0.9566.0.7688
C.....+x...+x......-x.....-3x
E.................0.8900.....
If initial CO is 9566 and equil CO is 0.8900, then x must be 0.9566-0.8900 = 0.0666.
Calculate CH4 = 0.6616+x for CH4, 0.8127+x for H2O, and 0.7688-3x for H2, substitute into the Kc expression and solve for Kc.

## Similar Questions

1. ### chemistry

The initial concentration for the compounds involved in the reaction displayed were determined to be [BrI(g)] = 0.3220 mol/L, [Br2(g)] = 0.3287 mol/L, [I2(g)] = 0.004086 mol/L. Calculate the value of the equilibrium constant (Kc) at …
2. ### chemistry(check my work)

The initial concentration for the compounds involved in the reaction shown were determined to be [CS2(g)] = 1.075 mol/L, [H2(g)] = 1.436 mol/L, [CH4(g)] = 0.6740 mol/L, [H2S(g)] = 0.3120 mol/L. Calculate the value of the equilibrium …
3. ### chemistry

I keep getting the wrong answer for this one can someone help. The initial concentration for the compounds involved in the reaction displayed were determined to be [NOCl(g)] = 0.1738 mol/L, [NO(g)] = 0.1991 mol/L, [Cl2(g)] = 0.000005938 …
4. ### chemistry

On this problem I keep getting the wrong answer. I am subtracting the initial concentration of Cl2 by the equilibrium concentration then using the difference to subtract for the rest using the mole ratios. Then i used the keq constant …
5. ### chemistry

The initial concentration for the compounds involved in the reaction displayed were determined to be [CH4(g)] = 0.9530 mol/L, [H2O(g)] = 0.9911 mol/L, [CO(g)] = 0.7474 mol/L, [H2(g)] = 0.2717 mol/L. Calculate the value of the equilibrium …
6. ### Chem

The initial concentration for the compounds involved in the reaction displayed were determined to be [NO2(g)] = 1.243 mol/L, [N2O4(g)] = 0.2578 mol/L. Calculate the value of the equilibrium constant (Kc) at 500.0 K if the equilibrium …
7. ### Chemistry

The initial concentration for the compounds involved in the reaction displayed were determined to be [PCl5(g)] = 0.4107 mol/L, [PCl3(g)] = 0.3463 mol/L, [Cl2(g)] = 0.04085 mol/L. Calculate the value of the equilibrium constant (Kc) …
8. ### General Chemisty

4. The initial concentration for the compounds involved in the reaction shown were determined to be [ClF(g)] = 0.5789 mol/L, [F2(g)] = 0.5980 mol/L, [Cl2(g)] = 0.05037 mol/L. Calculate the value of the equilibrium constant (Kc) at …
9. ### Chemistry

The initial concentration for the compounds involved in the reaction shown were determined to be [ClF(g)] = 0.5789 mol/L, [F2(g)] = 0.5980 mol/L, [Cl2(g)] = 0.05037 mol/L. Calculate the value of the equilibrium constant (Kc) at 2500 …
10. ### Chemistry

For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. I wrote: [N2O][H2O] / [NO]2 [H2] This reaction takes place at 25°C. At this temperature the concentration …

More Similar Questions