value: 0.80 points 15 attempts left Check my work Be sure to answer all parts. At 1000 K, a sample of pure NO2 gas decomposes: 2N02(g) 2NO(g) + O2(g) The equilibrium constant, Kp, is 158. Analysis shows that the partial pressure of O2 is 0.17 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture. Pressure of NO: □atm Pressure of NO2: atm Type here to search Esc F1 F2 F3

value: 0.80 points 15 attempts left Check my work Be sure to answer all parts. At 1000 K, a sample of pure NO2 gas decomposes: 2N02(g) 2NO(g) + O2(g) The equilibrium constant, Kp, is 158. Analysis shows that the partial pressure of O2 is 0.17 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture. Pressure of NO: □atm Pressure of NO2: atm Type here to search Esc F1 F2 F3

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 reaction: N₂O4 (9) 2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N2(g) + 202 (9) ⇒N₂O4(9) K₁ 1/2N₂(g) + O₂(g) NO₂ (g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K
Consider the equilibrium: 2 SO2(g) + O2(g) ⇄ 2 SO3(g) A student places 2.00 moles SO3 in a 1.00 L flask. When equilibrium is reached [O2] = 0.10 M at 130 °C. Calculate the Kc. Hint: use the detectivee method and construct an ICE table. Record your answer as a standard number to 2significant figures. For example, if the answer is 2.75 x 10-3 M then you should enter 0.00275 as the answer.
An equilibrium mixture contains 0.2500.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.2000.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g)+H2O(g)↽−−⇀CO2(g)+H2(g)CO(g)+H2O(g)⁢↽−−⇀⁢CO2⁢(g)+H2⁡(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.3000.300 mol once equilibrium has been reestablished? moles of CO2CO2 =
can you help the question?
Please provide the correct answer. We typically use ICE tables with these problems but I need help
At a certain temperature, the ?p for the decomposition of H2S is 0.770. H2S(g)↽−−⇀H2(g) + S(g) Initially, only H2S is present at a pressure of 0.268 bar in a closed container. What is the total pressure in the container at equilibrium? Ptotal= bar
Show work..don't give Handwritten answer....don't use Ai for answering this
Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375 X (b) What is Kp if the total pressure is 10.5 atm? 9.12
Consider the equilibrium 2NO(g)⇌N2(g)+ O2(g) For which ΔH = -180kJ mol-1 how will adding Xe(g) affect an equilibrium mixture of the three gases? a) Reactioj 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
▸ 69 20 E Consider the following system at equilibrium at 723 K: N₂(g) + 3H₂(g) 2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. D Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Removing H₂. C Submit Answer $ 4 R F % 5 V Retry Entire ♫ FS T G [References] the References to access important values if needed for this question. A 6 v yes no B MacBook Air F6 3 more group attempts remaining Y H & 7 B F7 U N * 8 00 D--ll FB J J ( T 1 M 9 K DD FO O O L ge A F10 P command Previous Email Instructor 4 i A AN = Next> Save and Exit ( { ? 912 option delete retu