A student ran the following reaction in the laboratory at 318 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) ? es if needed for this question. When he introduced CH₂Cl₂(9) at a pressure of 0.524 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CH₂Cl₂(g) to be 5.27x10-² atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining

A student ran the following reaction in the laboratory at 318 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) ? es if needed for this question. When he introduced CH₂Cl₂(9) at a pressure of 0.524 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CH₂Cl₂(g) to be 5.27x10-² atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining

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...

See similar textbooks

Similar questions

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -9 N, (g) + 2 H,0(g) =2H,(g) + 2NO (g) К, — 2. х 10 d. He fills a reaction vessel at this temperature with 7.0 atm of nitrogen gas and 3.2 atm of water vapor. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? x10 no If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. atm
A student ran the following reaction in the laboratory at 592 K:COCl2(g) CO(g) + Cl2(g)When he introduced COCl2(g) at a pressure of 0.510 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of COCl2(g) to be 0.201 atm.Calculate the equilibrium constant, Kp, he obtained for this reaction.Kp =
Suppose a 500. mL flask is filled with 0.60 mol of Br,, 0.10 mol of OCl, and 1.5 mol of BrOCl. The following reaction becomes possible: Br, (g) +OCl, (g) - - BrOC1(g) +Brci(g) The equilibrium constant K for this reaction is 0.349 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.7 mol of Br,, 1.4 mol of OCl, and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g)- BROC1(g)+BrC1(g) The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. olo ? Ar G Explanation Check © 2022 McGraw Hill LLC. AIL Rights Reserved. Terms of Use | Privacy Center | Accessibility
Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.300 mol N2 and 0.980 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)
A chemical engineer is studying the following reaction: CH,CH,NH,(aq)+HCl(aq) → Cl (aq)+CH,CH,NH;(aq) At the temperature the engineer picks, the equilibrium constant K¸ for this reaction is 0.92. The engineer charges ("fills") four reaction vessels with ethylamine and hydrogen chloride, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound concentration expected change in concentration vessel CH, CH,NH, 0.79 M f increase I decrease (no change) HCl 0.69 M f increase I decrease (no change) А Cl 0.62 M f increase I decrease (no change) CH,CH,NH, 0.81 M f increase I decrease O (no change) CH, CH,NH, 1.09 M f increase I decrease (no change) HCl 0.99 M f increase I decrease (no change)
A student ran the following reaction in the laboratory at 1080 K: 2SO3(9) 2SO₂(g) + O₂(g) When she introduced SO3(g) at a pressure of 1.16 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of O₂(g) to be 0.343 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
The equilibrium constant for the following reaction is K = 53.9 at a given temperature. If 1.21 mol of each H2 and I2 are placed in a 0.595 L flask, what is the concentration of H2 (molarity) at equilibrium? Report your answer to the thousandths place and do not include units. H2(g) + 12(g) = 2 HI(g)
the equilibrium constant K for the following reaction is 6.35 x 10: 2 HCl(g) At a certain temperature, H₂(g) + Cl₂(g) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.3 mol of H₂ and 1.3 mol of Cl₂. 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 3 significant digits. 2 HC1(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 H₂(g) + 3Cl₂(g) 6 HCl(g) There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2 (g) + 2 H,0(g) =2H,(g) + 2 NO (g) 8. :4. × 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? x10 no If you said yes, then enter the equilibrium pressure of NO at right. O Round your answer to 1 significant digit. atm
Consider the formation of phosphorus pentachloride from phosphorus trichloride and chlorine gas: PCl3 (g) + Cl2 (g) <---> PCl5 (g) If the equilibrium constant at a certain temperature is Kc = 1.36, what will the equilibrium concentration of PCl5 (g) be if the initial concentrations of the two reactant gases was each 0.450 M and that of the product was 0.100 M? (Note - the value of Q for the initial concentrations is 0.494, which is just a little below the value of Keq - although the reaction will proceed toward products, the final concentration of PCl5 will not increase very much).
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 1.5 L flask with 1.7 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.0 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K = [|