Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate equilibrium temperature.
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- If the equilibrium constant for an equilibrium system has decreased because of a "stress", how have the concentrations changed? O [reactants] and [products] decreases [reactants] decreases and [products] increases O [reactants] increases and [products] decreases [reactants] and [products] increasesarrow_forwardAmmonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 1.5 L flask with 3.0 atm of ammonia gas and 2.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.75 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. 0.8 Xarrow_forwardWhat can be said about the magnitude of the equilibrium constant in a reaction whose equilibrium lies far to the right? To the left?arrow_forward
- Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.arrow_forwardFor the reaction2NH3(g)+2O2(g)<=>N2O(g)+3H2O(g) the initial mixture contains 6.10 mol NH3 and 6.50 mol O2. At equilibrium, 1.75 mol of N2O gas are found. How many moles of NH3, O2, and H2O are present at equilibrium? Be sure to give your answers to two decimal places.______ mol NH3 ______ mol O2 ______ mol H2Oarrow_forwardAmmonia has been studled as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 2.0 L flask with 1.2 atm of ammonia gas and 1.4 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.36 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K ] Explanation Recheck 2021 McGraw-Hill Education. All Rights Reserved Tems of Use Privacy Accessarrow_forward
- Suppose the following exothermic reaction UO2(s)+4HF(g) UFA(g) + 2H20(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. State whether the equilibrium will shift to the reactants, will shift to the products, or will not be affected. Explain your answer using Le Chatelier's Principle. a. The system was cooled. b. The reaction vessel was quadrupled. C. Uranium (IV) oxide was added to the reaction. d. The partial pressure of Uranium (IV) fluoride was decreased.arrow_forwardThere are 5 main factors that affect the equilibrium of a chemical system.arrow_forwardDefine equilibrium constant Keqarrow_forward
- When the temperature of a system in equilibrium is decreased, what will happen to equilibrium? shifts towards absorbing heat reduces the number of moles increases the number of moles Shift towards releasing heatarrow_forwardIf Q is greater than K, the system will shift to the right to attain equilibrium. true or false?arrow_forwardAmmonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 1.5 L flask with 1.7 atm of ammonia gas and 2.1 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 0.77 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = ☐ P x10arrow_forward
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