Calculating equilibrium composition from an equilibrium constantSuppose a 250. mL flask is filled with 1.8 mol of CO, 1.3 mol of NO and 0.90 mol of CO2. The following reaction becomespossible:NO2(g)+CO(g) NO(g) + CO2(g)The equilibrium constant K for this reaction is 0.953 at the temperature of the flask.Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.Ом5?oloAr

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Answered: Calculating equilibrium composition…

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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O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 1.1: Cl₂(g) + CHCl3(g) → HCl(g) + CCl4(g) Use this information to complete the following table. Suppose a 8.0 L reaction vessel is filled with 0.35 mol of HCI and 0.35 mol of CCl4. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. HCl(g)+CC1,(9) Cl₂(9)+CHC13 (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 3 Cl₂(g) + 3 CHCl3(g) P 3 HCl(g)+3CCI (9) There will be very little Cl₂ and CHCl3. There will be very little HCI and CCI4. Neither of the above is true. K = 0 K = 0 x10 X 5 olo 18 Ar U
Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s) CaO(s) + CO₂(g) At a certain temperature, a chemist finds that a 2.8 L reaction vessel containing a mixture of calcium carbonate, calcium oxide, and carbon dioxide at equilibrium has the following composition: compound amount CaCO3 73.8 g CaO 42.1 g CO₂ 38.4 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = [0]
At a certain temperature, the equilibrium constant K for the following reaction is 3.44 x 10°: NO, (g) + CO(g)= NO(g) + CO,(g) Use this information to complete the following table. Suppose a 50. L reaction vessel is filled with 0.81 mol of NO2 and 0.81 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. x10 There will be very little NO and CO2. ? Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K =0 NO(g)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. = 0 K = 2 NO,(9)+2CO(9) 2 NO(9)+2CO2(9)
Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)–CaCO3(s) At a certain temperature, a chemist finds that a 5.4 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount CaO 11.0 g CO₂ 19.9 g CaCO3 64.3 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. 0 K 0 x10 X
Please answer with the correct number of significant digits. At a certain temperature, the equilibrium constant K for the following reaction is 9.7 x 10¹¹: NO₂(g) + CO(g) NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 42. L reaction vessel is filled with 1.2 mol of NO₂ and 1.2 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(9) 1 NO₂(9)+CO (9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 NO₂(9)+2CO(g) 1 2 NO(g) +2C0₂(9) There will be very little NO₂ and CO. There will be very little NO and CO₂. Neither of the above is true. K-O K-0 X
A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр
At a certain temperature, the equilibrium constant K for the following reaction is 6.09 × 10 °: N,(3) + O,(g) =2 NO(g) Use this information to complete the following table. Suppose a 28. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N2 and O2. There will be very little NO. 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 = ] 2 NO(g) N3(9)+O2(9) 1L What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2N2(9)+20,(9) 4 NO(g)
Consider the following equilibrium: NH3(g) + HCl(g) NH4CI(s) Suppose a vessel containing NH4Cl(s), NH3(g) and HCl(g) is at equilibrium. If the volume of the vessel is instantaneously doubled while keeping the temperature constant, when a new equilibrium is reached, which of the following statements is incorrect? The partial pressures of NH3 and HCI in the vessel remain unchanged. The total pressure is halved. O The value of Kp remains unchanged. O The number of moles of NH4Cl decreases. O The amount of NH3 and HCI doubles.
Suppose a 500. mL flask is filled with 0.10 mol of Br₂, 0.70 mol of OC12 and 0.40 mol of BrOC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) ⇒ BrOC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 7.81 at the temperature of the flask. Calculate the equilibrium molarity of BrOC1. Round your answer to two decimal places. M X S
Mercury and oxygen react to form mercury(II) oxide, like this: At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: 2 Hg(1)+O,(g)→2 HgO(s) compound amount 22.1 g Hg O2 24.2 g HgO 19.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
A student ran the following reaction in the laboratory at 316 K:2CH2Cl2(g) CH4(g) + CCl4(g)When he introduced CH2Cl2(g) at a pressure of 0.487 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be 0.219 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.

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