9:43 Question 10 of 17 For the reaction below, the partial pressure of NO₂ is 0.50 atm and the partial pressure of N₂O4 is 0.25 atm. What must happen for the reaction to reach equilibrium? 2 NO₂ (g) N₂O4 (g) Kp = 0.25 = A) The reaction needs to shift in the forward direction. Submit B) The reaction needs to shift in the reverse direction. C) The reaction is already at equilibrium and no shift needs to take place. D) There is not enough information to determine how the reaction will reach equilibrium. Tap here or pull up for additional resources

9:43 Question 10 of 17 For the reaction below, the partial pressure of NO₂ is 0.50 atm and the partial pressure of N₂O4 is 0.25 atm. What must happen for the reaction to reach equilibrium? 2 NO₂ (g) N₂O4 (g) Kp = 0.25 = A) The reaction needs to shift in the forward direction. Submit B) The reaction needs to shift in the reverse direction. C) The reaction is already at equilibrium and no shift needs to take place. D) There is not enough information to determine how the reaction will reach equilibrium. Tap here or pull up for additional resources

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

N204 (g) = 2 NO2 (g) N204 is placed into an empty container to an initial pressure of 1.292 atm at 219.0°C. After the reaction reaches equilibrium, the pressure of NO2 was 0.708. Assuming NO2 was only formed via the above reaction, calculate the value of Kp for the above reaction.
The following endothermic reaction is at equilibrium in a closed vessel. CaCO3(s)<-->CaO(s)+CO2(g) How will the equilibrium respond if we heat the system and raise its temperature by a thousand degrees? a) the new K is larger b) the new K is smaller c) K stays the same
At a particular temperature, Kp = 0.230 for the reaction N2O4(g) 2NO2(g) 1a) A flask containing only N2O4(g) at an initial pressure of 3.40 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 1b) With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.300 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
EXPLAIN STEP BY STEP
A reaction vessel initially contains 3.00 atm of SO2 and 1.00 atm of O2. A reaction occurs according to the equation: 2 SO2(g)+ O2(g) ⇄ 2 SO3(g)When equilibrium is reached, the total pressure is found to be 3.75 atm. What is the equilibrium constant Kp?
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
Given the reaction: A(s) B(g) + 2c(g) The total pressure at equilibrium is 4.20 atm. what is the value of Kp? O 12.6 O 9.48 O 16.4 O11.0 O 14.4
4. IBr decomposes according to the reaction at 150 C: 2 IB (g) = 12 (g) + Brz (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150°C? K = 8.3 x 10-3
Consider the reaction. 2 A(g) = B(g) Kp = 5.62 x 10-5 at 500 K If a sample of A(g) at 4.20 atm is heated to 500 K, what is the pressure of B(g) at equilibrium? PB = atm
A reaction vessel is charged with 0.50 atm of A and 0.300 atm of B. Once the reaction reaches equilibrium, what is the equilibrium partial pressure of B? Kp for this reaction is 67.2 A(g) - 2 B (g)
60) The following are the values of the equilibrium constant, K, for four different chemical reaction systems. For each of the chemical reaction systems, describe the equilibrium position of the given temperature as mostly products, mostly reactants, or equal concentrations of reactants and products. a) K= 10-12 at 25 °C