Consider the system below at equilibrium at 200°C:2Cl2 (g) + 2H20 (g) - 98.6KJ = 4HCI (g) + 02 (g)The change listed below would cause more reactants to form when equilibrium is re-established.Write A if true and B if false (Note: Answer is case sensitive)Addition of catalyst

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Answered: Consider the system below at…

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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Consider this system at equilibrium. A(aq) = B(aq) AH = -350 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q > K because Q increased. = K because neither changed. Q > K because K decreased. Q < K because K increased. О<к because Q decreased. How will the system respond to a temperature increase? shift right shift left no change
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
Determine the final temperature of a reaction that was initially 25 C, given that its equilibrium constant tripled and the reaction’s enthalpy of formation is 60.15 kJ/mol.
Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.
9) Given the following equilibrium reaction below, indicate which direction the reaction will shift when the indicated stresses are applied (à, ß, or none), AND indicate how the K value will change (increase, decrease or stays same) with the stress. P = 1 atm, unless otherwise specified. CO(g) + Cl2(g) ó COCl2(g) H = –107.6 kJ/mol What will happen if:ShiftK value i) The pressure is quadrupled________________________ ii) The reaction temperature is decreased_________________________ iii) More COCl2 gas is added_________________________ iv) The volume is doubled_________________________
Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g) <-----> 2H2O(g) + 2SO2(g) H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added
Consider the decomposition 4 PH3 (g) → P4 (s) + 6 H₂ (g) (Hrxn = -5.4 kJ/mol) Given the equilibrium constant for this process at 25°C is 233, what will be the value of the equilibrium constant at 37°C? (3 sf) Type your answer... of phosphene gas to form solid phosphorus and release hydrogen gas:

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Consider the system below at equilibrium at 200°C: 2C12 (g) + 2H20 (g) - 98.6KJ = 4HCI (g) + O2 (g) The change listed below would cause more reactants to form when equilibrium is re-established. Write A if true and B if false (Note: Answer is case sensitive) Addition of catalyst