Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Consider the reaction: CO(g) + Cl₂(g) COC12 (g) € Kp At equilibrium, this reaction is At equilibrium, the rates of→ and reaction are equal. At equilibrium, reactant and product concentrations are constant. Reactions continue after equilibrium has been reached. Decreasing the temperature changes the K, value for this reaction. Removing COC1₂(g) changes the value of K, for this reaction. For the reaction: COCI, (g) = CO(g) + Cl₂(g), the value of K, is equal to 6.7 x 10¹1 at 25°C V Varrow_forwardConsider the following equilibrium: 2NH₂ (g)-N₂ (g) + 3H₂(g) AG-34. KJ Now suppose a reaction vessel is filled with 4.85 atm of ammonia (NH3) a system: Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of H, will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of H₂ will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. and 2.40 atm of hydrogen (H₂) at 658. °C. Answer the following questions about this Ⓒrise O fall yes no atm 10 10 X Sarrow_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_forward
- If Q is greater than K, the system will shift to the right to attain equilibrium. true or false?arrow_forwardConsider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? 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 N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this Sarrow_forwardHeating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24arrow_forward
- Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 2.98×10-2 moles of COCl2, 0.206 moles of CO, and 0.304 moles of Cl2 are at equilibrium in a 17.8 L container at 672 K, the value of the equilibrium constant, Kp, is .arrow_forwardConsider the equilibrium, 2 NO (g) N2₂ (g) + O₂ (g), 2 for which AH = -180 kJ mol-1. How will adding more N₂ (g) affect an equilibrium mixture of the three gases? Select one: a. Reaction will proceed to the right (in the forward direction) to generate more product. b. Reaction will proceed to the left (in the reverse direction) to generate more product. C. Reaction will proceed to the right (in the forward direction) to generate more reactant. d. Reaction will proceed to the left (in the reverse direction) to generate more reactant. e. There will be no change to equilibrium mixture.arrow_forwardConsider the following equilibrium: 2NO, (g)–N,04 (8) AGº= – = - 5.4 kJ Now suppose a reaction vessel is filled with 5.06 atm of dinitrogen tetroxide (N,0) at 400. °C. Answer the following questions about this system: 2 rise Under these conditions, will the pressure of N,0, tend to rise or fall? 2 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can yes that be changed to a tendency to fall by adding NO,? Similarly, if you no said the pres of N,0, will tend to fall, can that be changed to a 2 4 tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits.arrow_forward
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