Predict the equilibrium partial pressure of HBr in the reaction described below by constructing an equilibrium expression for Qp, constructing an ICE table, writing the equilibrium constant expression, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure of HBr. Complete Parts 1-4 before submitting your answer. 2 HBr(g) = H:(g) + Br:(g) 1 2 3 4 NEXT > An initial mixture of 0.20 atm HBr, 0.010 atm Ha, and 0.010 atm Br: reacts. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qp.. Qp 5 RESET (0.20) (0.010) 2(0.20) 2(0.010) (0.20)? (0.010) 2(0.20) 2(0.010)? 5.0 x 104 0.050 0.0025 2.0 x 10 4.0 x 102

Predict the equilibrium partial pressure of HBr in the reaction described below by constructing an equilibrium expression for Qp, constructing an ICE table, writing the equilibrium constant expression, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure of HBr. Complete Parts 1-4 before submitting your answer. 2 HBr(g) = H:(g) + Br:(g) 1 2 3 4 NEXT > An initial mixture of 0.20 atm HBr, 0.010 atm Ha, and 0.010 atm Br: reacts. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qp.. Qp 5 RESET (0.20) (0.010) 2(0.20) 2(0.010) (0.20)? (0.010) 2(0.20) 2(0.010)? 5.0 x 104 0.050 0.0025 2.0 x 10 4.0 x 102

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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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H2S and 0.050 M SO2, what will the equilibrium concentration of H2O be? 2 H2S(g) + SO2(g)=3 S(s) + 2 H20(g) 1 NEXT > Based on the given values, set up ICE table in order to determine the unknown. 2 H2S(g) SO2(g) 3 S(s) 2 H20(g) + + Initial (M) |Change | (M) Equilibrium | (M) 5 RESET 0.050 +x +2x +3x -x -2x -3x 0.050 + x 0.050 + 2x 0.050 + 3x 0.050 - x 0.050 - 2x 0.050 -3x 0.025 + x 0.025 + 2x 0.025 + 3x 0.025 - x 0.025 - 2x 0.025 -3x
Predict the equilibrium concentration of Ca²+ in the reaction described below by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. NEXT > A solid sample of CaCrO dissolves in solution. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. 4 Initial (M) Change (M) Equilibrium (M) 7.1 x 104 - x 0 7.1 x 104 + 2x CaCrO₂(s) Ca²+(aq) + CrO²(aq) 1 CaCrO (s) 7.1 x 10-4 7.1 x 104 - 2x +X 2 11 -X Ca²+ (aq) +2x 3 + -2x CrO² (aq) RESET 7.1 × 10-¹4 + x
c) A mixture of H₂, I2 and HI is at equilibrium. Changes are made to the system, which then reaches a new equilibrium position. How will the concentrations of H₂ and HI at new equilibrium differ from their original concentrations when the following changes are made? Select: Increase, Decrease, or Unchanged i) 12(g) is removed from the reaction mixture [H₂] [HI] ii) Lower the temperature to 250°C at constant pressure (hint: the reaction is endothermic) [H₂] [HI]
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Predict the equilibrium partial pressure of HBr in the reaction described below by constructing an equilibrium expression for Qp, constructing an ICE table, writing the equilibrium constant expression, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure of HBr. Complete Parts 1-4 before submitting your answer. 2 HBr(g) = H₂(g) + Br₂(g) 2 3 NEXT > An initial mixture of 0.20 atm HBr, 0.010 atm H2, and 0.010 atm Br₂ reacts. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qp. (0.20) 5.0 x 10-4 (0.010) 0.050 1 Qp = 2(0.20) 0.0025 2(0.010) 2.0 × 10³ (0.20)² 4.0 x 10² = (0.010)² 4 2(0.20)² RESET 2(0.010)² +
The following reaction has an equilibrium constant of 2.65 x10-3 at 300K. Br2 (g) + Cl2 (g) 2 BrCl (g) Which of the following statements is true? Question 5 options: The system has a higher concentration of reactant molecules than product molecules at equilibrium, but there are significant quantities of both. The system consists almost entirely of reactant molecules at equilibrium. The system consists almost entirely of product molecules at equilibrium. The system has approximately equal concentrations of product and reactant molecules at equilibrium. The system has higher concentrations of product molecules than reactant molecules at equilibrium, but there are significant quantities of both.
HBr=.....M
The reaction of methane (CH 4) with Cl 2 forms chloroform (CHCl 3) and HCl. Although CHCl 3 is a general anesthetic, it is no longer used for this purpose since it is also carcinogenic. The molar masses for all substances are given under the balanced equation. CH4(g) + 3 Cl2(g) CHCl3(l) + 3 HCl(g) 16.04 g/mol 70.90 g/mol 119.4 g/mol 36.46 g/mol a. What is the theoretical yield of CHCl 3 in grams from 3.20 g of CH 4? b. What is the percent yield if 15.0 g of CHCl 3 are actually formed in this reaction?