7.8 When 0.210 moles of Br2 are placed into a sealed 0.800 dm³ flask at 1500 °C1.5% of the molecules dissociate. noBr2(g)prob2Br(g)a) Calculate the value of Kc at this temperature.b) What value of Kc do you expect if the total pressure of the system is doubled?250 dm3 was filled with 5.00 moles of NOCI and

Step 1: First let's calculate the dissociated moles of Br2:dissociated=(0.210mole…

Answered: 7.8 When 0.210 moles of Br2 are placed…

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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The reaction: Na, SO, • 10H20) + Na,SO(s)+10H2O() has a K, = 4.2r10 26 at 300.15K. What is its K.?
At 1000°C, the reaction NO2(g) + SO2(g) NO(g) + SO3(g) has K. = 5.94. Suppose 0.189 mol of NO2 and 0.189 mol of SO2 are placed in a 5.00 L container and allowed to react. Record all your answers to three (3) significant figures. What are the following concentrations at equilibrium? [NO2] = i M [SO2] = i [NO] = i M [SO3] = M eTextbook and Media
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A mixture of 0.03430 mol of C₂H6, 0.04797 mol of N₂, 0.01967 mol of NH3, and 0.02946 mol of C₂H4 is placed in a 1.0-L steel pressure vessel at 1257 K. The following equilibrium is established: 3 C₂Hg(9) + 1 N₂(g) 2 NH₂(g) + 3 C₂H4(9) At equilibrium 0.003643 mol of NH3 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of C₂H, N₂, NH3, and C₂H4. Peq(C₂H6)= Peg (N₂) = Peq(NH3)= Peg(C₂H4) (b) Calculate Kp for this reaction. Kp
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The equilibrium constant Kc for the reaction N2 + 3H2 = 2NH3 is 0.159 at 450°C. Calculate the equilibrium composition when 1.50 mol N2 is mixed with 4.50 mol H2 in a 5.00 L vessel. [N2] = %3D M [H2] = %3D M [NH3] = M
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