Nitrogen dioxide decomposes according to the reaction: 2 NO2(g) = 2 NO(g) + O2(g) where Kp = 4.48 x 10-8 at a certain temperature. If 0.565 atm of NO2 is added to a container and allowed come to equilibrium, what is the equilibrium partial pressure of NO? (the answer should be entered with 3 significant fiçures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) Question 17 of 31 A Moving to another question will save this response. MacBook Air 20, esc %23 % & * 3 5 6. 7 W R Y tab F K caps lock C V B alt command option option command V LL 24 A

Nitrogen dioxide decomposes according to the reaction: 2 NO2(g) = 2 NO(g) + O2(g) where Kp = 4.48 x 10-8 at a certain temperature. If 0.565 atm of NO2 is added to a container and allowed come to equilibrium, what is the equilibrium partial pressure of NO? (the answer should be entered with 3 significant fiçures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) Question 17 of 31 A Moving to another question will save this response. MacBook Air 20, esc %23 % & * 3 5 6. 7 W R Y tab F K caps lock C V B alt command option option command V LL 24 A

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

Give handwritten answer
4NH3(g) +50₂(g) = 4NO(g) + 6H₂O(g) AH = -1000. kJ K = 1.35 The equilibrium concentrations are [NH3] = 0.20M, [02] = 0.90M, [H2O] = 1.34 M, and [NO] = [?] What is the equilibrium concentration of NO at 25 °C? [NO] M Enter
At a certain temperature, Keq = 135.5 for the following equilibrium: SO2(g) + NO2(g) <===> NO(g) + SO3(g) Suppose a reaction vessel at this temperature contained these three gases at the following concentrations: [SO2] = 0.00250 M, [NO2] = 0.00350 M, [NO] = 0.0250 M, [SO3] = 0.0400 M. a)Determine Qeq for the system. (b)Is the system at equilibrium? If it is not, indicate the direction toward which the system will move to reach equilibrium.
For the equilibrium 3H₂(g)+N₂(g) P -0.00239 atm, P," NH₂ -0.763 atm and P 2NH, (g), the equilibrium partial pressures are = 0.921 atm, at 500°C. Calculate Kp.
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:
4. Toluene, C;H8(1), is an important organic solvent. It is made industrially from methylcyclohexane, C,H14(g): C,H14(g) + heat ? 2C;H8(1) + 3H2(g) State three different changes to an equilibrium mixture of these reacting gases that would shift the reaction toward greater production of toluene. State and explain each change.
Please don't provide handwritten solution ...
please indiciate whether the pressure will decrease, increase, or not change. Also please indicate what the shift in equilibrium will be
A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =
Methanol is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g) + 2 H2(g) <-> CH3OH(g). At equilibrium mixture in a 1.05 L vessel is found to contain 0.652 mol CH3OH, 0.386 mol CO, and 0.209 mol H2. Calculate the value of Kc.
10