# Chemistry

posted by .

A sealed 1.0L flask is charged with .500mol I2 and .500mol Br2 and an equilibrium reaction esues: I2(g)+Br2(g)=2IBr(g)
When the container contents achieve equilibrium, the flask contains .84 mol of IBr. What is the value of the eqilibrium constant? (K)

• Chemistry -

I2(g)+Br2(g)=2IBr(g)
I .500 .500 0

C -x -x +2x

E .500-x .500-x .84

I know K=[product]/[reactant] but I don't know what to do with the information from there.

• Chemistry -

Never mind I figured it out

• Chemistry -

ths results cm 4rm table..products/reactants..(84)^2/(416)^2(416)^2

## Similar Questions

1. ### chem 203

Br2=2Br When 1.05 mol of br2 is placed in a .950L flask, 1.20% of Br2 undergoes dissociation. Calculate the equilibrium constant Kc, for this reaction. Use ICE table.
2. ### chem class

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)(equilibrium arrow) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.46 …
3. ### chemistry

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)(equilibrium arrow) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.46 …
4. ### AP CHEMISTRY

For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.590 mol IBr in a 2.50-L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2?
5. ### AP CHEMISTRY

I've got another question. it's similar to this but this time with Kp. Here's the question: For the equilibrium 2IBr(g) <-> I2(g) + Br2(g) Kp = 8.5 10-3 at 150.°C. If 0.016 atm of IBr is placed in a 2.5-L container, what is …
6. ### Chemistry

After 4.00 mol of C2H4(g) and 2.50 mol of Br2 (g) are placed in a sealed 1.0L container, the reaction reaches equilibrium and is written following: C2H4(g) + Br2(g) -> C2H4Br2(g) ... Calculate the equilibrium concentrations of all …
7. ### chemistry

A 0.10-mol sample of H2(g) and a 0.10-mol sample of Br2(g) are placed in a 2.0-L container. The reaction H2(g) + Br2(g) <----> 2 HBr(g) is then allowed to come to equilibrium. A 0.20 mol sample of HBr is placed into a second …
8. ### chem

For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.570 mol IBr in a 2.50-L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2?
9. ### chemistry

At a certain temperature, Keq is 4.13 x 10^-5 for the equilibrium: 2IBr(g) ↔ I2(g) + Br2(g) Assume that the equilibrium is established at the above temperature by adding only the reactant to the reaction flask. What are the concentrations …
10. ### chemistry

Consider the following reaction in the solvent CCl4 in a 1-L flask: 2IBr(g)<->Br2(g)+I2(g) What is the equilibrium moles of IBr, Br2 and I2 are 0.2, 0.1 and 0.1, calculate the equilibrium constant Kc.

More Similar Questions