QUESTION 17 Ammonia gas is produced by the reaction between nitrogen gas and hydrogen gas in a closed 250 cm container. Equilibrium is reached at 400 °C according to the following chemical equation Nzie) + 3H2ie) > 2NH3) Initially 3mol of N2) was injected into the container with an unknown amount of Hzie) - When equilibrium was established it was found that 2,2mol of NH3() was present while 1,5mol of He) remained in the container. 17.1 Determine how many moles of H24) were used up in the reaction. (2) 17.2 determine how many moles of N2e) was present at equilibrium. (2) 17.3 Determine the amount of Hziej in moles present at the start of the reaction. (2) 17.4 Write the expression for the equilibrium constant K, for the reaction (2) 17.5 Calculate the value of the equilibrium constant K, for this reaction at 400 °C (5) END

QUESTION 17 Ammonia gas is produced by the reaction between nitrogen gas and hydrogen gas in a closed 250 cm container. Equilibrium is reached at 400 °C according to the following chemical equation Nzie) + 3H2ie) > 2NH3) Initially 3mol of N2) was injected into the container with an unknown amount of Hzie) - When equilibrium was established it was found that 2,2mol of NH3() was present while 1,5mol of He) remained in the container. 17.1 Determine how many moles of H24) were used up in the reaction. (2) 17.2 determine how many moles of N2e) was present at equilibrium. (2) 17.3 Determine the amount of Hziej in moles present at the start of the reaction. (2) 17.4 Write the expression for the equilibrium constant K, for the reaction (2) 17.5 Calculate the value of the equilibrium constant K, for this reaction at 400 °C (5) END

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...

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Dinitrogen tetroxide was used as part of the fuel for the lunar lander in the Apollo missions. It establishes the equilibrium below. N2O4 (g) <--> 2 NO2 (g) Kp = 0.133 If an unknown pressure of N2O4 was added to a reaction flask, and 90.0% of the N2O4 still remains once equilibrium has been established, what was the initial pressure that was added to the reaction flask?
Question 1 1 Consider the following reaction at 425 °C: H2 (g) + I2 (g) = 2HI(g) An equilibrium mixture contains 1.22 x 10-2 mol H2, 1.22 x 10-2 mol I2 and 9.00 x 10-2 mol HI in a 5.00 L reactor. At a certain instant, a valve is opened, and 1.40 × 10-2 mol of I2 is added to the reactor. 1.1 Determine the value of Ke at 425 °c 1.2 Once equilibrium has been re-established, the concentration of hydrogen iodide gas in the reactor was measured to be 2.03 x 10-2 M. Determine the concentration of the other species present in the system for this set of conditions.
2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g) You have 0.4 moles C2H2 and 0.2 moles O2 present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process? Question 5 options: Conc. C2H4 O2 CO2 H2O Initial 0.4 0.2 0 0 Change -x -x +x +x Equil. 0.4-x 0.2-x x x Conc. C2H4 O2 CO2 H2O Initial 0.08 0.04 0 0 Change -2x -5x +4x +2x Equil. 0.08-2x 0.04-5x 4x 2x Conc. C2H4 O2 CO2 H2O Initial 0.4 0.2 0 0 Change -2x -5x +4x +2x Equil. 0.4-2x 0.2-5x 4x 2x Conc. C2H4 O2 CO2 H2O Initial 0.08 0.04 0 0 Change -20x -20x +20x +20x Equil. 0.08-20x 0.04-20x 20x 20x
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N, (g) + 2H,0(g)=2 NO(g) + 2H, (g) K,=2. × 10-9 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 1.9 atm of water vapor. Use this data to answer the questions in the table below. yes Can you predict the equilibrium pressure of H2, using only the tools x10 available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.
Please explain why the answer you get is correct. Thank you very much for all of your help!
Which statements below best describe a chemical system at homogeneous equilibrium? 1. The reactants and products have the same concentration 2. The rate of the forward reaction stops 3. The concentration of reactants and products remain constant O Statement Il only O Statement I only Statement III only Statements I and III « Previous Next
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Question 19
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N,0,(g)=2 NO,(e Three experiments were run starting with different initial amounts of N,O4(g) ([N,O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO, and N,04 at equilibrium. Be sure to round to the correct number of significant figures. Exp N,0,lo NO,l N,0, NO,] / N,04] 2 [NO,] / N,04 NO,1 / [N,04] 1 3.5 2.85 2.1 2 3.0 2.56 1.7 3 2.1 2.06 1.1 Based on your calculations, indicate whether each statement is True (T) or False (F): ♥1. Each experiment started with a different initial concentration of N,O4. v 2. The ratio ([NO,]/NO1) is equal to a constant value. v3. The ratio (2 [NO,] / [N,041) is…