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, 0.960 mol SO, is placed in a 2.50 L container. 2 SO, (g) = 2 SO,(g) + 0,(g) At equilibrium, 0.190 mol O, is present. Calculate K. K. =arrow_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_forwardNonearrow_forward
- General Chemistry 4th Edition McQuarrie Rock Gallogly University presentedi The equilibrium constant for the chemical equation N,(g) + 3 H, (g) =2 NH,(g) is K, = 0.139 at 237 °C. Calculate the value of K. for the reaction at 237 °C. Ke =arrow_forwardAt -9.76 °C the concentration equilibrium constant K = 5.3 × 105 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 11.%. • If the reaction is run at constant pressure, 64.0 kJ/mol of heat are released. • The net change in moles of gases is - 1. Using these facts, can you calculate K at 15. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether K at 15. °C will be bigger or smaller than K at -9.76 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. O No. 0 x10 Xarrow_forwardAt room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).arrow_forward
- Steam reforming of methane ( CH,) produces "synthesls gas," a mixture of carbon monoxlde gas and hydrogen gas, which Is the starting polnt for many 4 Important industrial chemical syntheses. An Industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of methane gas and 2.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.1 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = || Check Explanation 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessib M 9 hp Cearrow_forwardating UP bunE Ammonia 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 liquld form It is easily transported. An Industrial chemist studying this reaction fills a 200. mL flask with 1.6 atm of ammonia gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.7 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 = Check Explanation 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility M 9 hp escarrow_forwardConsider the following reaction: 2HI(g) = H2 (g) + I2 (g) If 2.99 moles of HI(g) , 0.359 moles of H2, and 0.628 moles of I2 are at equilibrium in a 19.6 L container at 859 K, the value of the equilibrium constant, Kc , is .arrow_forward
- At a certain temperature, 0.660 mol SO, is placed in a 2.50 L container. 2 SO; (g) = 2 SO,(g)+ 0,(g) At equilibrium, 0.130 mol O, is present. Calculate K. Kearrow_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_forwardConsider the following equilibria at a given temperature: ½Nalg) + J½O>(g) = NO(g) K= 6.45 x 10°, NO (g) + 1½Brz(g) = NOB((g) K= 1.40 Determine the value of the equilibrium constant for the following reaction at the same temperature: %N(g) + ½Ozlg) + ½Br2(g) = NOBr(g) OA 583 x 107 O B.3.36 x 10-18 OC4.17x 107 OD.6.45 x 10 OE 9.03 x 10arrow_forward
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