Knowee
Questions
Features
Study Tools

2. Given the following information, use an ICE table to calculate the equilibrium concentration of BrCl.[Br2]i = 0.225[Cl2]i = 0.125Kc = 0.0875Br2(g)+ Cl2(g) ⇌ 2BrCl(g)0.104 M0.050 M0.204 M0.153 M

Question

  1. Given the following information, use an ICE table to calculate the equilibrium concentration of BrCl.[Br2]i = 0.225[Cl2]i = 0.125Kc = 0.0875Br2(g)+ Cl2(g) ⇌ 2BrCl(g)0.104 M0.050 M0.204 M0.153 M
🧐 Not the exact question you are looking for?Go ask a question

Solution

The ICE table stands for Initial, Change, and Equilibrium. It's a table that's used to calculate the equilibrium concentrations of reactants and products in a chemical reaction. Here's how you can use it to solve this problem:

  1. Write down the balanced chemical equation:

    Br2(g) + Cl2(g) ⇌ 2BrCl(g)

  2. Set up the ICE table. The initial concentrations are given as [Br2]i = 0.225 M and [Cl2]i = 0.125 M. Since no initial concentration is given for BrCl, we can assume it's 0.

    Br2 Cl2 BrCl
    Initial 0.225 0.125 0
    Change -x -x +2x
    Equil. 0.225-x 0.125-x 2x

  3. Write the equilibrium expression using the law of mass action (Kc = [products]/[reactants]):

    Kc = [BrCl]^2 / ([Br2][Cl2]) = 0.0875

  4. Substitute the equilibrium concentrations from the ICE table into the equilibrium expression:

    0.0875 = (2x)^2 / ((0.225 - x)(0.125 - x))

  5. Solve this equation for x. This is a quadratic equation, and you can use the quadratic formula to solve it.

  6. Once you have the value of x, substitute it back into the equilibrium row of the ICE table to find the equilibrium concentrations of Br2, Cl2, and BrCl.

Please note that solving the quadratic equation might be complex and you might need to use a calculator or a software to get the exact value of x.

This problem has been solved

Similar Questions

a. At a certain temperature, Kc is 4.13 x 10 -2 for the equilibrium:2 IBr (g) I2 (g) + Br2 (g)Assume that equilibrium is established at the above temperature by adding only IBr (g) to the reactionflask. What are the concentrations of I2 (g) and Br2 (g) in equilibrium with 0.0124 moles/liter of IBr(g) ?

Given the following information, use an ICE table to calculate the value of Kc.[NO]i = 0.261 M[Cl2]i = 0.364 M[NOCl]eq = 0.123 M2NO(g) + Cl2(g) ⇌ 2NOCl(g)2.630.2630.026326.3

Consider the chemical system:2 NO(g) + Br2(g)  ⇋ 2 NOBr (g)K = 2.0  How do the equilibrium concentrations of the reactants compare to the equilibrium concentration of the product?Question 2Select one:a.You can't tell from the information givenb.They are much higherc.They have to be exactly equald.They are about the same order of magnitudee.They are much lower

Suppose a 500.mL flask is filled with 0.30mol of Cl2, 0.40mol of CHCl3 and 1.5mol of CCl4. The following reaction becomes possible:+Cl2gCHCl3g +HClgCCl4gThe equilibrium constant K for this reaction is 8.88 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.

A solution is made by mixing 30.0 mL of 0.150M (mol/L) compound A with 25.0 mL of 0.200M (mol/L) compound B. At equilibrium, the concentration of C is 0.0454M. Calculate the equilibrium constant, K, for this reaction.A (aq) + 2B (aq) <---> C (aq)The initial concentrations of A and B are not 0.150 M and 0.200 M

1/3

Upgrade your grade with Knowee

Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.