Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What effect will adding additional O2 (g) to the following equilibrium system have, once equilibrium is reestablished? 2 CO2 (g) 2 CO (g) + O2 (g) ∆H ̊ = -514 kJ
a) The concentration of CO(g) will increase
b) The concentration of CO2 (g) will decrease
c) The equilibrium constant for the reaction will increase
d) The concentration of CO2 (g) will increase
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- 101edu.co b For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.230 atm. What is AG for this reaction? (R = 8.314 J/mol-K). 1 Q 2 W 3 E $ 4 R % 5 T Question 12 of 12 A 6 & 7 Presen 8 Home ( 9 End Carrow_forwardNitrogen and oxygen react at high temperatures. N2(g) + O2(g) 2 NO(g) ΔH = 182.6 kJ (b.) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added? If more O2 is added, [N2] ---Select--- increases decreases remains the same , [O2] ---Select--- increases decreases remains the same , and [NO] ---Select--- increases decreases remains the same . (c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? If N2 is removed, [N2] ---Select--- increases decreases remains the same , [O2] ---Select--- increases decreases remains the same , and [NO] ---Select--- increases decreases remains the same . (d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added? If more NO is added, [N2] ---Select--- increases decreases remains the same , [O2] ---Select--- increases decreases remains the same , and [NO] ---Select--- increases decreases remains the same .…arrow_forwardH2(g) + Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? ○ The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieve ○ The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achievedarrow_forward
- explain step by step.arrow_forwardConsider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases. B. decreases. C. remains the same. The value of Q fill in the blank 2 A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: fill in the blank 3 A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The concentration of H2 will: fill in the blank 4 A. increase. B. decrease. C. remain the same.arrow_forwardNitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no changearrow_forward
- You are given the following: H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011 H2 (g) 2 H (g) Kp = 4.8 x 10-41 Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below? H (g) + Br (g) HBr (g) Kp = ?arrow_forwardDry ice (solid carbon dioxide) is placed in a sealed container. It sublimes to produce carbon dioxide gas and reaches equilibrium at a given temperature. If the amount of dry ice in the container is doubled, then _____________. (After choosing the correct answer justify why in your own words why you chose that answer) CO2 (s) = CO2 (g) A)The amount of CO2 (g) would double. B)The amount of CO2 (g) would increase but not double. C)The amount of CO2 (g) would not change. D)The equilibrium amount of CO2 (s) would be less.arrow_forwardConsider the following endothermic reaction: 4 PCl5 (g) ⇋⇋ P4 (s) + 10 Cl2 (g) How will the amount of Cl2 be affected if the total pressure of the system is increased? Select one: a. The concentration of Cl2 will increase. b. The concentration of Cl2 will decrease. c. The amount of Cl2 will not change.arrow_forward
- For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.270 atm. What is AG° for this reaction? (R = 8.314 J/mol · K). kJ/mol 1 3 4 C 7 8 9 +/- x 100 + 2.arrow_forward(a) N2(g) + O2(g) 2NO (g) ∆H298 = + 180 kJ mol-1 From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by: Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalystarrow_forward
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