Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- At a certain temperature, the equilibrium constant K for the following reaction is 6.8 x 10°: Cl,(e) + CHCI, (g). - HC1(g) + CC1,(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 0.70 mol of HCl and 0.70 mol of CCI4. What can you say about the composition of the O There will be very little Cl2 and CHCI3. mixture in the vessel at equilibrium? O There will be very little HCl and CCl4. O 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 =|| HCl(g)+CCl,(9) Cl,(0)+CHC13(0) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = | 3 Cl,(0)+3CHC13(g) 3 HCl(g)+3CC14(9)arrow_forwardHydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) H,(g) + Cl,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.73 М H2 1.2M Cl2 0.90M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = [] %3D 10 Explanation Check O 2022 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center Access DELL Esc F1 F2 F3 F4 F5 U F6 F7 F8 F9 F10 F11 F12 PrtScr Insert Delete "R # $ & Num Lock 1 2 3 4 Backspace 7 Tab R Y * 00arrow_forwardO KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a partial equilibrium... 0/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 21. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.3 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 IIarrow_forward
- Picturearrow_forwardHydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) - H2(9) + Cl,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.49 M H, 1.9M Cl, 0.10M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K̟ = 0arrow_forward8) Consider the system below. When equilibrium is restored, how will the number of each type of molecule and the concentration of each substance compare to those before the stress was introduced? Complete the following table using the words "decrease," "same," or "increase." 2 NH,(g) = N,(g) + 3 H,(g) AH = 92.4 kJ/mol Decrease Volume Decrease Temperature N, Equilibrium Concentration Н, NH, N, Equilibrium Number Н, NH,arrow_forward
- A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 3 H₂(g) ⇒ 2 NH3 (g) K₂=8.x 10-7 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 6.8 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. Oyes O no atm 10 Xarrow_forward3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.arrow_forwardA chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 3 H₂ (g) 2 NH₂ (g) K₂= 6. × 10¯6 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 2.4 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. yes no atm x₁ x10 × Śarrow_forward
- At a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g) 3BrOCl (g) +3BrCl (garrow_forwardFor the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.arrow_forwardTrue/False. Explain your answer in one sentence or less. In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.arrow_forward
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