When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H₂O(g) = CO2(g) + H₂(g) + heat For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the products, shifts in the direction of the reactants, or does not change. Drag the appropriate items to their respective bins. removing some CO₂(g) adding more H₂(g) adding more H₂O(g) Shifts in the direction of the products decreasing the volume of the container Shifts in the direction of the reactants Reset chill the reaction Equilibrium does not change Help

When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H₂O(g) = CO2(g) + H₂(g) + heat For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the products, shifts in the direction of the reactants, or does not change. Drag the appropriate items to their respective bins. removing some CO₂(g) adding more H₂(g) adding more H₂O(g) Shifts in the direction of the products decreasing the volume of the container Shifts in the direction of the reactants Reset chill the reaction Equilibrium does not change 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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. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2
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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
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7) N2(g) + 2O2(g) ------> In the endothermic equilibrium reaction of 2NO2(g), how does the equilibrium system change and in which direction does the equilibrium move when the following operations are performed? a) When the volume is increased, b) When the Cl2 concentration is reduced, c) When the temperature is increased,