Hydrogen gas and bromine gas are mixed in a sealed container at 250°C and allowed to reachequilibrium.H2(g) + Br2(g)= 2HB1(g)The equilibrium constant for this reaction at 250°C is 65.5.At equilibrium, the concentration of H2 is 0.0510 mol L*1 and the concentration of Brris0.174 mol L-1 at 250°C.(i) Write the equilibrium constant expression for the above reaction.(ii) Calculate the concentration of HBr in the equilibrium mixture at 250°C(iii) Explain what happens to the concentration of HBr you calculated in (ii) above if the pressure ofthe equilibrium mixture is increased.

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Answered: Hydrogen gas and bromine gas are mixed…

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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At a certain temperature, the equilibrium constant K for the following reaction is 3.44 x 10°: NO, (g) + CO(g)= NO(g) + CO,(g) Use this information to complete the following table. Suppose a 50. L reaction vessel is filled with 0.81 mol of NO2 and 0.81 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. x10 There will be very little NO and CO2. ? Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K =0 NO(g)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. = 0 K = 2 NO,(9)+2CO(9) 2 NO(9)+2CO2(9)
Consider the reaction shown below at room temperature. 2H2(g) + S2(g) ⇋ 2H2S(g) The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S. (a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?
The equilibrium constant, K, for the following reaction is 83.3 at 500 K. PCI,(2) + Cl,(g)=PCI<(g) Calculate the equilibrium concentrations of reactant and products when 0.352 moles of PCl, and 0.352 moles of Cl, are introduced into a 1.00 L vessel at 500 K. [PCI,] =[ M [C)] M [PC!g] = [ M
At a certain temperature, the equilibrium constant K for the following reaction is 6.09 × 10 °: N,(3) + O,(g) =2 NO(g) Use this information to complete the following table. Suppose a 28. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N2 and O2. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2 NO(g) N3(9)+O2(9) 1L What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2N2(9)+20,(9) 4 NO(g)
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) +You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, andthe concentration of NH3 is 0.85 M.(a) Calculate the value of the reaction quotient Q.(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed toreach equilibrium.
An important step in the industrial production of hydro- gen is the reaction of carbon monoxide with water: CO(g) + H2O(g) = CO2(g) + H2(g) (a) Use the law of mass action to write the equilibrium expression for this reaction. (b) At 500°C, the equilibrium constant for this reaction is 3.9. Suppose that the equilibrium partial pressures of CO and H,O are both 0.10 atm and that of CO, is 0.70 atm. Calculate the equilibrium partial pressure of H2(g).
Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G
A chemical engineer is studying the following reaction: 2 NO(g)+2H2(g) → N,(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.17. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound pressure expected change in pressure NO 3.80 atm f increase CI decrease (no change) H2 5.43 atm f increase I decrease (no change) А N2 7.72 atm f increase I decrease (no change) H,0 3.07 atm f increase C+ decrease (no change) NO 4.19 atm f increase I decrease (no change) H, 5.64 atm f increase I decrease (no change) В N2 6.22 atm f increase I decrease (no change) H,0 1.83 atm f increase I decrease (no change) NO 3.39…
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)
The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.40 M , and [C] = 0.300 M. The following reaction occurs and equilibrium is established: %3D %3D A + 2B = C At equilibrium, [A] = 0.270 M and [C = 0.430 M. Calculate the value of the equilibrium constant, K. Express your answer numerically. • View Available Hint(s) ΑΣφ Kc =
LRererencesj Isoidan 1 Use the References to access important values if needed for this question. Consider the following equilibrium system at 844 K. 2HI(8) 2 H2 (g) + L (g) If an equilibrium mixture of the three gases at 844 K contains 0.196M HI, 3.37 × 10-2 M H2, and 2.80 × 10- M I2, what is the value of the equilibrium constant K?

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