If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established C(s) + H20(g) = CO(g) + H2(g) You may use each option more than once Removing H2(g) 1. Forward Removing carbon 2. Reverse Adding H20(g) 3. No change Adding carbon > >

If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established C(s) + H20(g) = CO(g) + H2(g) You may use each option more than once Removing H2(g) 1. Forward Removing carbon 2. Reverse Adding H20(g) 3. No change Adding carbon > >

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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5. Calculate the concentration of the products of the following equilibrium when the equilibrium constant is 12.3 and the equilibrium concentration of NOBr₂ is 2.17 mol/L. NOBr₂ (g) NO(g) + Br₂(g) Answer: Submit your completed Assignment Booklet to Moodle at the end of this lesson.
Part A Consider the following reaction in chemical equilibrium: COC1₂ (g) CO(g) +Cl₂ (g) What is the effect of adding additional CO(g) to the reaction mixture? What is the effect of adding additional COC12 (g)? Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. Submit right Cl₂ CO left COC12 Request Answer < Return to Assignment Adding COC2 increases the concentration of progress to shift to the Adding CO increases the concentration of to shift to the (away from the Provide Feedback " " |). Reset causing the reaction Help causing the reaction progress
Consider this reaction with K-11.8 A (g) + B (g) 2C (g) Initially there is 0.524 atm of reactant A, 0.524 atm of reactant B, and no C present. What is the partial pressure of product C at equilibrium? A) 0.662 atm B) 0.937 atm C) 0.607 atm D) 0.556 atm E) 0.788 atm
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d. Suppose you add compound E to the equilibrium mixture. Compound E reacts with compound D which is a component of the equilibrium to form compound F as described in the equation below. E + D Which compound is removed from the equilibrium mixture when you add compound E to the mixture? (Enter "correct" for ALL correct answers.) • B D e. What shift in the equilibrium will occur as a result of the addition of compound E? (Enter "correct" for the correct shift.) A + B C + D (shift to the right) A + B C + D (shift to the left)
* Question Completion Status: QUESTION 1 Consider the following reversible reaction at equilibrium: 3 H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the reactants (left side)? O Decreasing the amount of NH3. O Adding a catalyst to the system. O Decreasing the volume of the system. O Decreasing the temperature. O Decreasing the amount of H2. QUESTION 2 Click Save and Submit to save and submit. Click Save All Answers to save all answers. arch DELL prt sc FIO DII F9 F8 F3 F4 FS
Consider the reaction below. 3.28 mol of A and 10.5 mol of B are added to a 3.00 L container. At equilibrium, the concentration of A is 0.743 M. What is the concentration of at equilibrium? (complete chart) 1 A + 2 B ↔↔ 3 C --------- 1 A + 2 B ↔↔ 3 C Initial M M M Change - M - M + M Equilibrium 0.743 M M M Use the concentrations above to calculate the equilibrium constant for this reaction: Keq = ?
3. Assume that the following exothermic reaction is at equilibrium H 2(g) + I 2(g) = 2 HI(g) Tell whether the position of equilibrium will shift to the right or the left if we: Remove some HI Add some I2 Increase the pressure Increase the temperature Add a catalyst
22) The ke for the equilibrium shown below is 45. Some methane and hydrogen sulfide are added to a container and at equilibrium the concentrations of methane and hydrogen sulfide are found to be 0.22 mol/L and 0.33 mol/L respectively. What are the equilibrium concentrations of carbon disulfide and hydrogen gas? CH4 + 2H2S(g) → CS2 (g) 4H2
14. The following reaction is allowed to come to equilibrium and then the volume is increased. Predict the effect of the indicated volume change once equilibrium is restored. H2O(g) + CO2(g) double arrow H2CO3(g) The reaction will shift right. The reaction will shift left. There will be no effect. Effect can not be determined from information provided.
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