# chemistry

posted by .

The equilibrium constant Kc for the reaction

C <--> D + E

is 7.90 * 10^-5. The initial composition of the reaction mixture is [C]=[D]=[E]=1.10*10^-3. What is the equilibrium concentrations of C, D, and E?

C=?
D=?
E=?

• chemistry -

K = 7.9E-5 = (D)(E)/(C)
Qc = (0.0011)(0.0011)/(0.0011) = 0.0011
Qc > Kc; therefore, products are too large and reactants too small. The reaction most go to the left to reach equilibrium.

..........C ==> D ...+... E
I......0.0011..0.0011..0.0011
C.........x.....-x.......-x
E...0.0011+x..0.0011-x.0.0011-x

Substitute the equilibrium line from the ICE chart into Kc expression and solve for x, then 0.0011+x and 0.0011-x.

## Similar Questions

1. ### Chemistry

SO this is my first time doing this... lol i need help on an AP chemistry question for equilibrium. A 0.500 L tank contains 3.00 g of NO(g) at 750. K. The equilibrium constant for the reaction below at this temperature is 3.4 x 10 …
2. ### chemistry

For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, …
3. ### chemistry

For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, …
4. ### chemistry

For the reaction H2(g) + I2(g) ¡ê 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change …
5. ### chemistry

The equilibrium constant Kc for the reaction C <--> D + E is 7.90 * 10^-5. The initial composition of the reaction mixture is [C]=[D]=[E]=1.10*10^-3. What is the equilibrium concentrations of C, D, and E?
6. ### Chemistry

Consider the reaction HCHO(g) *) H2(g) + CO(g). 1.0 mol of HCHO, 1.0 mol of H2 and 1.0 mol of CO exist in equilibrium in a 2.0 L reaction vessel at 600C. a) Determine the value of the equilibrium constant Kc for this system. 2.0 moles …
7. ### Chemistry

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 ✕ 103. 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) If the initial concentration of NO is 0.160 M, what are the equilibrium concentrations of NO, …
8. ### chemistry

A reaction is represented by this equation: 2W( aq ) ⇌ X( aq ) + 2Y( aq ) K c = 5 × 10 −4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of ≤1 M , make up two sets of …
9. ### chemistry

A reaction is represented by this equation: 2W( aq ) ⇌ X( aq ) + 2Y( aq ) K c = 5 × 10 −4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of ≤1 M , make up two sets of …
10. ### Chemistry

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a specific temperature with initial concentrations of [CO] = 0.27 M and [H2] = 0.49 M. At equilibrium, the concentration of CH3OH is 0.11 …

More Similar Questions