Canvas POF SOU-CCJ230-Introd... Problem-Solving Strategies: Understanding Equilibrium▼ Part A Identify the stressConsider the equilibrium reactionCO(g) + H₂O(g) - CO₂(g) + H₂(g)Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response.Drag the appropriate labels to their respective targets.► View Available Hint(s)Increase reactantDecrease reactantIncrease productDecrease productSubmitType here to searchReverse reaction ratetemporarily increasesForward reaction ratetemporarily increasesForward reaction ratetemporarily decreasesReverse reaction ratetemporarily decreasesChangeAdd CO(g)Remove H₂O(g)Add CO₂(g)Remove H₂(g)IHSystem stressGroup 1Group 1Group 1Group 1✔CaEquilibrium shiftGroup 2Group 2Group 2Group 2ResetHelp

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em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

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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7:40 i 65% on.masteringchemistry.com :D The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = K.(RT)An 0.08206 L · atm/(K· mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction where R N2(g) + 3H2(g) = 2NH3 (g) for which An = 2 – (1+ 3) = -2. Part A For the reaction 3A(g) + 2B(g)= C(g) Kc = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s)