The equilibrium constant, K, for the following reaction is 10.5 at 350 K.2CH,Cl,(g) CH4(g)+ CC14(g)An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.16x10-² M CH,Cl,, 0.167 M CH, and0.167 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.75x10-2mol of CH,Cl,(g) is added to the flask?(CH,Cl,] =M[CH4)M%3D[CC4]MThe equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K.NH,I(s) NH3(g) + HI(g)An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.222 mol NH,I, 8.37×103M NH3 and 8.37×10-³ M HI. If the concentration of NH3(g) is suddenly increased to 1.34×10-² M, what will be theconcentrations of the two gases once equilibrium has been reestablished?[NH3] =M[HI]M

Given, 2CH2Cl2g↔CH4g+CCl4g Volume = 1L CH2Cl2eq=5.16 X 10-2MCH4eq = 0.167 MCCl4eq=0.167 Mmoles of…

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH,Cl½(g)#CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.16×10-² M CH,Cl,, 0.167 M CH4 and 0.167 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.75×10² mol of CH,Cl½(g) is added to the flask? (CH,Cl,] = M [CH4) M (CC!] M The equilibrium constant, K, for the following reaction is 7.00×10*5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.222 mol NH¼I, 8.37×103 M NH3 and 8.37×10-³ M HI. If the concentration of NH3(g) is suddenly increased to 1.34×10² M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI] = M

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH,Cl½(g)#CH4(g) + CC14(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.16×10-² M CH,Cl,, 0.167 M CH4 and 0.167 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.75×10² mol of CH,Cl½(g) is added to the flask? (CH,Cl,] = M [CH4) M (CC!] M The equilibrium constant, K, for the following reaction is 7.00×10*5 at 673 K. NH,I(s) NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.222 mol NH¼I, 8.37×103 M NH3 and 8.37×10-³ M HI. If the concentration of NH3(g) is suddenly increased to 1.34×10² M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M (HI] = 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...

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