**Equilibrium System at 298 K****Chemical Reaction:**\[ \text{2NO(g) + Br}_2\text{(g)} \leftrightharpoons \text{2NOBr(g)} \]**Scenario:**If the **PRESSURE** of the equilibrium system is suddenly increased at constant temperature:### Reaction Behavior**The reaction must:**1. [Dropdown Option] A. Run in the forward direction to reestablish equilibrium.2. [Dropdown Option] B. Run in the reverse direction to reestablish equilibrium.3. [Dropdown Option] C. Remain the same. Already at equilibrium.### Number of Moles of Br₂**The number of moles of Br₂ will:**1. [Dropdown Option] A. Increase.2. [Dropdown Option] B. Decrease.3. [Dropdown Option] C. Remain the same.

According to Le Chatlier principle, if the pressure of the equilibrium system is suddenly increased,…

Consider the following system at equilibrium at 298 K: 2NO(g) + Br2(g) 2NOBr(g) If the PRESSURE of the equilibrium system is suddenly increased at constant temperature: A. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The number of moles of Br, will: A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium at 298 K: 2NO(g) + Br2(g) 2NOBr(g) If the PRESSURE of the equilibrium system is suddenly increased at constant temperature: A. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The number of moles of Br, will: A. Increase. B. Decrease. C. Remain the same.

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

Consider the following system at equilibrium where AH° = -16.1 kJ, and K, = 154 , at 298 K: 2 NO (g) + Br2 (g) :2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly increased : The value of K.A. Increases B. Decreases C. Remains the same The value of Q.JA. Is greater than K. B. Is equal to K, C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will:DA. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium at 350 K: ? CHĄ(g) + CCl4(g) 2CH,Cl,(g) When some CCI,(g) is removed from the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CH4 will: | A. Increase. B. Decrease. C. Remain the same.
Consider the equilibrium 2NO(g)⇌N2(g)+ O2(g) For which ΔH = -180kJ mol-1 how will adding H2(g) affect an equilibrium mixture of the three gases? a) Reaction will proceed to the left to generate more reaction b) reaction will proceed to the right to generate more product c) there will be no change to the equilibrium mixture
12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as follows: A (g) + 3B (g) = C (g) + 2D (g) a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x, and the equilibrium concentrations al all the reactants and produces with respect to x. b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B, C, and D. c. Calculate the value for the equilibrium constant at this temperature.
Which of the following equilibrium systems will shift to the right (toward the products) when pressure isincreased? A. 2 PbS(s) + 3 O2(g) ⇋ 2 PbO(s) + 2 SO2(g)B. PCl5(g) ⇋ PCl3(g) + Cl2(g)C. H2(g) + CO2(g) ⇋ H2O(g) + CO(g)D. All of these will shift to the right.E. None of these will shift to the right.
d. he following system establishes an equilibrium at 545 K: NH₂HS (s)- NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a b. The volume of the container is doubled. The temperature of the system is raised to 825 K C. Some additional solid NH4HS is added. The reaction flask has 1.25 atm of the inert gas argon added to it. 5. (10 points) At 355 K, a 10.00 L reaction flask is charged with 1.44 atm each of hydrogen and fluorine gas. The following reaction takes place: H2 (8) + F2 (g) = 2 HF (g) Kp = 176 Based on building an ICE table, determine the partial pressure of H2, F2 and HF once equilibrium has been established.
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: The reaction must: 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 I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
10. For the reaction at equilibrium H2(g) + CO2(g): = H2O(g) + CO(g) Kc = 0.10 at 420°C Which statement is true? a . Slightly more H2O and CO is present than H2 and CO2. b. Slightly more H2 and CO2 is present than H2O and CO. C The reaction vessel contains mostly CO and H2O. d. The reaction vessel contains mostly CO2 and H2O.
The system below was at equilibrium in a 7.0 L container. What change will occur for the system when the container is shrunk to 2.5 L? 2SO₂(g) + O₂(g) = 2SO3(g) + 198 kJ Hint: How many moles of gas are on each side? A. There is no change because there are the same number of moles of gas on both sides. B. The reactions shifts to the left (reactants) to produce more moles of gas. C. The reactions shifts to the right (products) to produce fewer moles of gas.
Answers are attached. Please show all steps and make an ICE table. Thank you!
Consider the following reaction: NO(g) + SO3(g) = NO2(g) + SO2(g) A reaction mixture initially contains 0.639 M NO and 0.639 M SO3. Determine the equilibrium concentration of NO2 if K, for the reaction at this temperature is 0.0118. Enter the numerical value to three decimal places without units. Answer: