The equilibrium constant, K₉, for the following reaction is 9.52×10⁻² at 350 K.\[ \text{CH}_4 \, (\text{g}) + \text{CCl}_4 \, (\text{g}) \rightleftharpoons 2 \, \text{CH}_2\text{Cl}_2 \, (\text{g}) \]Calculate the equilibrium concentrations of reactants and product when 0.289 moles of CH₄ and 0.289 moles of CCl₄ are introduced into a 1.00 L vessel at 350 K.\[ [\text{CH}_4] = \boxed{\hspace{1cm}} \, \text{M} \]\[ [\text{CCl}_4] = \boxed{\hspace{1cm}} \, \text{M} \]\[ [\text{CH}_2\text{Cl}_2] = \boxed{\hspace{1cm}} \, \text{M} \] ### Equilibrium Concentration CalculationThe equilibrium constant, \( K_c \), for the following reaction is **10.5** at **350 K**.#### Reaction:\[ 2 \text{CH}_2\text{Cl}_2 (g) \rightleftharpoons \text{CH}_4 (g) + \text{CCl}_4 (g) \]#### Problem:Calculate the equilibrium concentrations of reactant and products when **0.328 moles** of \(\text{CH}_2\text{Cl}_2\) are introduced into a **1.00 L** vessel at **350 K**.#### Equilibrium Concentrations:- \([\text{CH}_2\text{Cl}_2]\) = \([ \, ] \, \text{M}\)- \([\text{CH}_4]\) = \([ \, ] \, \text{M}\)- \([\text{CCl}_4]\) = \([ \, ] \, \text{M}\)

The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K. CH4 (g) + CC14 (g)=2 CH2C12 (g) Calculate the equilibrium concentrations of reactants and product when 0.289 moles of CH4 and [ CH4] [ CC4] M M

The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K. CH4 (g) + CC14 (g)=2 CH2C12 (g) Calculate the equilibrium concentrations of reactants and product when 0.289 moles of CH4 and [ CH4] [ CC4] M M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The equilibrium constant, Ke, for the following reaction is 10.5 at 350 K. 2CH,Cl2(g)CH,(g) + CC14(g) =CH¾(g) + CC1¼(g) Calculate the equilibrium concentrations of reactant and products when 0.374 moles of CH2C1, are introduced into a 1.00 L vessel at 350 K. [CH2C2] =| M [CH4] M [CCL4] M ||
1) Given the following reaction what is the expression for K? 2SO2 (g) + 02 (g) = 2S03 (g)
A student ran the following reaction in the laboratory at 1097 K: 2SO3(g)2SO2(g) + O2(g) When she introduced 0.0921 moles of SO3 (g) into a 1.00 liter container, she found the equilibrium concentration of O₂ (g) to be 0.0198 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
2) Based on the information below, determine the value of the unknown equilibrium constant, Kc. 2 NOCl (g) « 2 NO (g) + Cl2 (g)Kc = 2.4 x 10-7 1/3 Cl2 (g) + 2/3 NO (g) « 2/3 NOCl (g)Kc = ?
A student ran the following reaction in the laboratory at 281 K: 2 CH2CI2 (g) CH4 (g) + CCI4 (g) When she introduced 7.87x102 moles of CH2CI2 (g) into a 1.00 liter container, she found the equilibrium concentration of CCI4 (g) to be 3.68×102 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =
10
3. Given the chemical reaction A(aq) + 2B(aq) → C(aq) + 3D(aq) Initially, you have 2 moles of A and 3 moles of B dissolved in a total volume of 3 L. a. X moles of A reacted, and the solution reached equilibrium. Solve for the End state in term of x b. Write down the expression of the equilibrium constant (Keq) in term of x and volume.
Consider the reaction: Important values if I for this question C(s) + O₂(g) → CO₂(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: C(s) + 1/2O₂(g) → CO(g) K₁ CO(g)+1/2O,(g)=CO2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K =
Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: (3)H+(3)0ɔ= (3)0°H+(3)0) The equilibrium constant K for this reaction is 0.735 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. OM
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N₂(g) + O₂(g) 2NO(g) Ke=4.3 × 10-25 2NO(g) + O₂(g) = 2NO₂(g) K=6.4 × 10⁹ Determine the value of the equilibrium constant for the following equation at the same temperature: N₂(g) +20₂(g) = 2NO₂(g) Ke= 10 (Enter your answer in scientific notation.)
N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =