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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Write the equilibrium constant expression, K., for the following reaction: If either the numerator or denominator is 1, please enter 1 N2 (g) + 3 H2 (g)=2 NH3 (g) K. =
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.
The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCI2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.232 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = M [CO] M [Cl,] M
A student ran the following reaction in the laboratory at 566 K: CO(g) + Cl2(g) = COC2(g) When she introduced 0.655 moles of CO(g) and 0.680 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of COCI,(g) to be 0.618 M. Calculate the equilibrium constant, K, she obtained for this reaction. Ke
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
A student ran the following reaction in the laboratory at 375 K: CH4(g) + CC14(g) = 2CH2C22(g) When she introduced 4.58x10 2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
A student ran the following reaction in the laboratory at 322 K: 2NO(g) + Br2(g) = 2NOB1(g) When she introduced 0.107 moles of NO(g) and 9.86×102 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBR(g) to be 7.65x102 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =

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