A student ran the following reaction in the laboratory at735 K:N2(g) + 3H2(g) = 2NH3(g)When she introduced 0.0402 moles of N2 (g) and 0.0547moles of H2(g) into a 1.00 liter container, she found theequilibrium concentration of NH3 (g) to be 0.000861 M.Calculate the equilibrium constant, Kc, she obtained forthis reaction.Кс=

Given:The volume of the container = 1.00 L (3 significant figures)Initial moles of…

Answered: A student ran the following reaction in…

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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Use the References to access important values if needed for this question. Consider the following reaction: 2NOBrig)2NO(g) + Bry(g) If 0.342 moles of NOBR(g), 0.396 moles of NO, and 0.547 moles of Br, are at equilibrium in a 12.9 L container at 510 K, the value of the equilibrium constant, K, is Retry Entire Group 9 more group attempts remaining Submit Answer Next Previous Email Instructor Save and Exit 7:45 PM 77°F Mostly cloudy 10/11/2021 ho brt sc delete home 9. backspace lack
A student ran the following reaction in the laboratory at 431 K: PCI5 (g) = PCI3 (g) + Cl2 (g) When she introduced 2.91 moles of PCI5 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl2 (g) to be 3.70x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc
The equilibrium constant, Kc, for the following reaction is 6.30 at 723 K. 2NH3 (9) ⇒ N₂ (9) + 3H₂ (9) If an equilibrium mixture of the three gases in a 12.8 L container at 723 K contains 0.496 mol of NH3(g) and 0.448 mol of N₂, the equilibrium concentration of H₂ is M.
A student ran the following reaction in the laboratory at 282 K: 2NO(g) + Br2(g) = 2NOBr(g) When she introduced 0.170 moles of NO(g) and 0.137 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.135 M. Calculate the equilibrium constant, K., she obtained for this reaction. K.
Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr.
A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II
The equilibrium constant, Ke, for the following reaction is 1.51×102 at 635 K. 2HI(g) H2(g) + I½(g) When a sufficiently large sample of HI(g) is introduced into an evacuated vessel at 635 K, the equilibrium concentration of I2(g) is found to be 0.414 M. Calculate the concentration of HI in the equilibrium mixture. M
At 27 °C, K, = 1.5 × 1018 for the reaction 3NO(g) = N20(g) + NO2(g) If 0.030 mol of NO were placed in a 1.00 L vessel and equilibrium were established, what would be the equilibrium concentrations of NO, N20, and NO2. [NO] = M [N20] = M [NO2] = M
A student ran the following reaction in the laboratory at 286 K:2CH2Cl2(g) CH4(g) + CCl4(g)When she introduced 6.64×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.09×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Kc =
The equilibrium constant, Kc, for the following reaction is 1.39 at 663 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 663 K, the equilibrium concentration of H₂(g) is found to be 0.957 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = = M
A student ran the following reaction in the laboratory at 377 K: CH₂(g) + CCL (9) ⇒ 2CH₂Cl2 (9) When she introduced 0.0391 moles of CH4 (g) and 0.0708 moles of 14 CCl4 (g) into a 1.00 liter container, she found the equilibrium concentration of CCl4 (g) to be 0.0623 M. Calculate the equilibrium constant, Ko, she obtained for this reaction. Kc =
A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…

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