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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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A flask is filled with 1.50 M NO2. After reaching equilibrium according to the reaction below, the concentration of NO is 0.35 M. What is the equilibrium constant?
2NO2 (g) ⇌ 2NO (g) + O2 (g)
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- CO (g) + 2 H2 (g) ⇌ CH3OH (g) How many grams of CO does it need to react with 4 moles of H2? 14.00 g 28.01 g 56.02 g 112.04 garrow_forwardAt equilibrium the concentrations of N2 , H2 and NH3 are 4.0 M, 8.0 M and 4.6 M, respectively. Find the initial concentrations of N2 and H2 given that Kc is equal to 1.20 x 102. N2 (g) + 3H2 (g) ⇌ 2 NH3 (g)arrow_forwardCarbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g), Kc=5.50 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium?arrow_forward
- Consider a hypothetical chemical reaction: A(g) ⇌ 3B(g) You put 1.00 mol of gas B in a 50.0 L container, seal it and wait for the reaction to reach equilibrium. At equilibrium you find 0.25 mol of gas A in the container. What is the K value for this reaction?arrow_forwardWrite the mathematical expression for the reaction quotient, QP, for each of the following reactions (we prefer to use partial pressure as concentration unit for gases) : 1. 2NH3(??) ⇌ N2(??) + 3H2(??) 2. 2NO(??) + Cl2(??) ⇌ 2NOCl(??)arrow_forwardFor the reaction below, Kc = 7.2 × 10⁻⁴. What is the equilibrium concentration of NOF if the reaction begins with 0.92 M NO and 0.92 M F₂? 2 NO (g) + F₂ (g) ⇌ 2 NOF (g)arrow_forward
- For the reaction below, Kc = 4.60 × 10⁻⁶. Note Kc is sometimes called K. What is the equilibrium concentration of B if the reaction begins with 0.400 M A? A (g) ⇌ 3 B (g)arrow_forwardAt a particular temperature, 12.0 moles of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) At equilibrium. 3.0 moles of SO2 is present Calculate K for this reaction.arrow_forward2 NO2(g) + 87 kJ ⇌ 2 NO(g) + O2(g) Which of the following will cause the concentration of NO2(g) to increase in the above reaction? Choose all that apply Increasing the pressure of the system Decreasing the temperature of the system Decreasing the concentration of NO (g) Increasing the volume of the systemarrow_forward
- 1. At a certain temperature, the value of K for the following reaction is 4.2 x 10. N₂(g) + O₂(g) → 2NO(g) 0.45 mol of nitrogen gas and 0.26 mol of oxygen gas are put in a 6.0 L reaction vessel. What is the equilibrium concentration of NO (g) at this temperature? Clearly show your stepsarrow_forwardIn which direction does the following equilibrium shift when the gas mixture is compressed? Explain using Le Châtelier’s principle and in terms of forward and reverse reaction rates. 2 C(s) + O2(g) ⇌ 2 CO(g)arrow_forwardKc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430 ° C. Calculate the equilibrium concentrations of H2, I2, and HI at 430 ° C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.485 M. [H2] = M [I2] = M [HI] = Marrow_forward
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