A chemical engineer is studying the following reaction:CH₂(g) + 2H₂S(g) → CS₂(g) + 4H₂(g)At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³.рThe engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, and lets the reaction begin. He then measures the composition of themixture 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.reactionvesselABcompoundCH4H₂SCS₂H₂CHAH₂SCS₂H₂pressure5.65 atm3.56 atm5.77 atm7.93 atm4.69 atm1.62 atm6.73 atm11.81 atmOOexpected change in pressure↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increaseolo↓decrease↓decrease↓ decrease↓decrease↓ decrease↓decrease↓ decrease↓ decrease(no change)(no change)(no change)(no change)(no change)(no change)(no change)(no change) reactionvesselABCcompoundCHAH₂SCS₂2H₂CHA4H₂SCS₂2#2CH4H₂SCS,H₂pressure5.65 atm3.56 atm5.77 atm7.93 atm4.69 atm1.62 atm6.73 atm11.81 atm5.53 atm3.31 atm5.89 atm8.44 atmexpected change in pressure↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↑ increase↓ decrease↓ decreasedecrease↓ decrease↓decrease↓ decrease↓ decrease↓ decrease↓ decreasedecrease↓ decreasedecrease(no change)(no change)(no change)8(no change)(no change)(no change)(no change)O(no change)(no change)(no change)(no change)(no change)

A chemical engineer is studying the following reaction: CH4(9)+2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. P The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, 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 vessel A B compound CH4 H₂S CS₂ H₂ CH4 H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm expected change in pressure † increase ↑ increase Ot increase Ot increase Ot increase Ot increase ↑ Ot increase ↑ increase O decrease Odecrease Odecrease Odecrease decrease Odecrease Odecrease Odecrease (no change) O(no change) O(no change) (no change) (no change) (no change) O(no change) (no change)

A chemical engineer is studying the following reaction: CH4(9)+2H₂S(g) → CS₂(g) + 4H₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.7 × 10³. P The engineer charges ("fills") four reaction vessels with methane and hydrogen sulfide, 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 vessel A B compound CH4 H₂S CS₂ H₂ CH4 H₂S CS₂ H₂ pressure 5.65 atm 3.56 atm 5.77 atm 7.93 atm 4.69 atm 1.62 atm 6.73 atm 11.81 atm expected change in pressure † increase ↑ increase Ot increase Ot increase Ot increase Ot increase ↑ Ot increase ↑ increase O decrease Odecrease Odecrease Odecrease decrease Odecrease Odecrease Odecrease (no change) O(no change) O(no change) (no change) (no change) (no change) O(no change) (no change)

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

3. For the reaction SO2(g) + NO2(g) 2 NO(g) + SO3(g), Ko = 85.0 at 4.60 x 102 °C. A reaction is started with 0.0500 M of both reactants (Note, initially no products). a) Calculate the equilibrium concentration in M of all species. (If you correctly set-up the ICE chart for this problem, you will see the equilibrium constant expression is a perfect square & so the quadratic formula is not needed. If yours is not a perfect square, check your work.)
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N(g) + 2 H,O(g) = 2H,(g) + 2 NO(g) K, = 2. × 10¯° He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 2.9 atm of water vapor. Use this data to an yes Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. atm
A chemical engineer is studying the following reaction: N(g)+3 H,(9) - 2 NH;(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0016. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 pressure expected change in pressure vessel 11.39 atm Of increase O I decrease O (no change) H. 25.28 atm O t increase OI decrease O (no change) A NH, 16.95 atm O t increase OI decrease O (no change) 12.82 atm O t increase OI decrease O (no change) 28.45 atm O f increase OI decrease O (no change) B NH, 21.46 atm O f increase O I decrease O (no change) N 10.92 atm O f increase OI decrease O (no change) O I decrease O (no change) H. 23.86…
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 chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.33. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound H₂ C1₂ HC1 H₂ CL, HCl H₂ CL₂2 HC1 pressure 4.42 atm 5.14 atm 1.90 atm 3.61 atm 4.33 atm 3.53 atm 4.59 atm 5.31 atm 1.57 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓decrease ↓decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no…
At a certain temperature, the equilibrium constant K for the following reaction is 5.36 x 10": H,(g) + Cl,(g) = 2 HCI(g) Use this information to complete the following table. Suppose a 33. L reaction vessel is filled with 0.63 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little H2 and Cl2. O There will be very little HCI. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = ] 2 HCl(g) H,(9)+Cl,(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = ] 2 H,(9)+2Cl,(9) 4 HCl(g) Continue O 2022 McGraw Hill LLC. All Rights Reserve 43,203 FEB 18 9 PP SESS
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 7.45 × 10-5: NO₂(g) + CO(g) ⇒ NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 20. L reaction vessel is filled with 1.5 mol of NO and 1.5 mol of CO₂. 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. NO(g)+CO,(9) NO₂(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 NO₂(g) + 3 CO(g) P 3 NO(g)+ 3 CO₂(9) There will be very little NO2 and CO. There will be very little NO and CO₂. Neither of the above is true. K = 0 K = 0 x10 Ś ? ollo 18 Ar BA
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 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 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, = 0
A chemical engineer is studying the following reaction: H₂(g)+I₂(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant The engineer charges ("fills") three reaction vessels with hydrogen and iodine, 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 vessel A B C compound H₂ 1₂ HI H₂ 1₂ HI H₂ 1₂ HI pressure 2.39 atm 3.83 atm 4.71 atm 2.82 atm 4.26 atm 3.85 atm 3.81 atm 5.76 atm 5.21 atm expected change in pressure ↑ increase increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase for this reaction is 1.2. р ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease X (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no change)…
A chemical engineer is studying the following reaction: H,(g)+L,(g) 2 HI(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.0. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, 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 vessel compound pressure expected change in pressure H, 2.86 atm O 1 increase O (no change) decrease 2.34 atm O t increase OI decrease O (no change) HI 1.38 atm O f increase decrease O (no change) H, 2.45 atm O t increase decrease O (no change) 1.93 atm O t increase O I decrease o (no change) B O t increase O (no change) HI 2.21 atm decrease 2.75 atm O t increase o (no change) H, decrease 2 23 atm O t Increase decrease O (no change) HI O T increase decrease…
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 500. mL flask with 1.2 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 0.60 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, -0 x10 5
At a certain temperature, the equilibrium constant K for the following reaction is 575.: H₂(g) + 1₂(g) → 2 HI(g) Use this information to complete the following table. Suppose a 44. L reaction vessel is filled with 0.64 mol of HI. 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 HI(g) H₂(9) + 1₂ (9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 H₂(g)+31₂(9) 6 HI(g) There will be very little H₂ and 12. There will be very little HI. Neither of the above is true. K = 0 -0 K =