Use K and initial concentrations to calculate equilibrium concentrations.Consider the equilibrium system involving the decomposition of nitrogen monoxide.[N2] [02]2NO(g)?N2(g) + O2(g)K ==2.78×10-2 at 287 K[NO]²A flask originally contains 0.378 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases.[NO] ==[N2][02]=Σ Σ ΣMCheck & Submit AnswerShow Approach

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Answered: Use K and initial concentrations to…

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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2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) The system initially contained 0.2500 M NO, 0.1300 M H2, and 0.2500 M H₂O. At equilibrium, the concentration of NO is 0.1296 M. What is the equilibrium concentration of H₂? [H₂] = [?] x 10¹ M K= [N₂] [H₂O]2 [NO]2[H₂]2 Coefficient (green) Exponent (yellow) Enter
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N2O4(g) 2 NO2(g) Three experiments were run starting with different initial amounts of N2O4(g) ([N2O4]0 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 NO2 and N2O4 at equilibrium.Be sure to round to the correct number of significant figures. Exp [N2O4]0 [NO2] [N2O4] [NO2] / [N2O4] 2 [NO2] / [N2O4] [NO2]2 / [N2O4] 1 3.7 2.92 2.2 2 2.8 2.49 1.6 3 2.6 2.33 1.4 Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N2O4. 2. The…
Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G
Say that you mix Fe3+ and SCN- together so that after mixing, the concentration of Fe3+ (aq) equals 0.0015 M , and the concentration of SCN- (aq) equals 5.5 x 10-4 M. You measure the concentration of product, FeSCN2+, after equilibrium forms. It is 7.2 x 10-5 M. Calculate the value of the equilibrium constant, K, for the reaction. F e 3 + ( a q ) + S C N − ( a q ) ⟷ F e S C N 2 + ( a q ) K = ? Group of answer choices 0.011 9.52 x 10-3 87.3 105
Consider the following equilibrium: 2NOCl (g) <--> 2NO (g) + Cl2 (g) With K = 1.6 x 10-5. 1.00 mole of pure NOCl and 0.964 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of Cl2 (g).
Consider the following reaction: 2 AB(g) = 2 A(g) + B2(g) The reaction is allowed to proceed until equilibrium is reached, and the final concentrations are: [AB] = 0.041 M [A] = 0.061 M [B2] = 0.030 M %3D %3D %3D Calculate the value of the equilibrium constant, K. Enter the numerical value using 2 significant figures.
An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =
3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.
CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g) K = 7.3@823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H2O. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).

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