Consider the following reaction that is at equilibrium in a sealed vessel: A(g) + B(g) + C(s) = 2D(g) Which of the following statements are true? Decreasing the volume of the container to one half its original volume will shift the reaction to the right. Decreasing the volume of the container to one half its original volume will shift the reaction to the left. Decreasing the volume of the container to one half its original volume will not cause a shift the reaction to either direction. Increasing the amount of C in the vessel will change the amount of D(g) present once equilibrium is re-established. If the concentration of B is increased, the concentration of A will be lower after equilibrium is re-established.

Consider the following reaction that is at equilibrium in a sealed vessel: A(g) + B(g) + C(s) = 2D(g) Which of the following statements are true? Decreasing the volume of the container to one half its original volume will shift the reaction to the right. Decreasing the volume of the container to one half its original volume will shift the reaction to the left. Decreasing the volume of the container to one half its original volume will not cause a shift the reaction to either direction. Increasing the amount of C in the vessel will change the amount of D(g) present once equilibrium is re-established. If the concentration of B is increased, the concentration of A will be lower after equilibrium is re-established.

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

10) For the reaction: 2 V PC13(g) + Cl2(g) → PC15(g) at 85°C, Kp = 1.19 = If one starts with 2.00 atm pressure of PC13, 1.00 atm pressure of Cl2 and no PC15, what is the partial pressure of PC15(g) at equilibrium? A) 0.739 atm B) 0.621 atm C) 0.465 atm D) 0.167 atm E) 0.553 atm
Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + 02 (g) AH° = -514 kJ Le Châtelier's principle predicts that adding additional O2 (g) from the reaction container will A) The reaction will shift to decrease the pressure. B) The reaction will shift in the direction of the reactants. . C) The reaction will shift in the direction of the products. D) The equilibrium constant will decrease. E) No change in the reaction
The following reaction is exothermic. 2 NO(g) + 2 H2(g) ⇔ N2(g) + 2 H2O(g) In which direction does the equilibrium shift as a result of each of the following changes? Here are the possible answers: to the right, to the left, no effect Place these actions in chronological order. Space 1: The hydrogen gas is removed. Space 2: The gas pressure in the reaction vessel is increased by decreasing its volume. Space 3: The gas pressure in the reaction vessel is increased by pumping argon gas into it while keeping the volume constant. Space 4: We raise the temperature. Space 5: A catalyst is used.
7. Please refer to the attached photo. Thank you!!
Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At equilibrium, [NOCl] = 1.60 M and [NO] = 0.80 M. The [Cl2] is
Consider the following reaction where K, = 55.6 at 698 K. H2(g) + I2(g) =2HI(g) A reaction mixture was found to contain 2.94×102 moles of H2(g), 4.25×102 moles of I2(g) and 0.301 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
Iron and water react to form iron (III) oxide and hydrogen, like this: 2 Fe(s)+3 H₂O(g)→Fe₂O3(s)+ 3 H₂(9) At a certain temperature, a chemist finds that a 8.1 L reaction vessel containing a mixture of iron, water, iron (III) oxide, and hydrogen at equilibrium has the following composition: compound amount Fe 1.92 g H₂O 1.12 g Fe₂03 2.32 g H₂ 2.30 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 X
Question 4 of 25 Submit The equilibrium constant for the reaction 2 HF (g) = H2 (g) + F2 (g) is 0.270 at a particular temperature. What is the equilibrium constant for the equation ½ H2 (g) + ½ F2 (g)= HE (g)? 1 3 C 7 9. +/- x 10 0 LO 00
4
Consider the following reaction where Kc = 55.6 at 698 K.H2(g) + I2(g) 2HI(g)A reaction mixture was found to contain 4.52×10-2 moles of H2(g), 4.50×10-2 moles of I2(g) and 0.298 moles of HI(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionfill in the blank 2A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium. Submit Answer
Iron and water react to form iron (III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) →Fe₂O3(s)+3H₂(g) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount Fe 3.39 g H₂O 2.88 g Fe₂O3 2.96 g H₂ 3.61 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K 0 X ?
Consider the general reaction: 2A(g) + B(g) = 2C(g) If the equilibrium pressures for each substance are: A = 2 atm B = 3 atm C = 1 atm What is the value of K,? None of these are correct. O 0.083 0.16 O 12