### Chemical Equilibrium Questions1. **Problem Statement and Reaction:** - In an experiment, 0.30 mol H₂ and 0.30 mol I₂ are mixed in a 1.00-L container, and the reaction forms HI. If \( K_c = 49 \) for this reaction, what is the equilibrium concentration of HI? \[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g) \]2. **Multiple Choice Question:** - Which of the following is true for a system whose equilibrium constant is much smaller than one? a. The reaction mixture contains mostly reactants at equilibrium. b. The reaction mixture contains mostly products at equilibrium. c. The rate of reaction is very slow. d. The moles of reactants and products are relatively similar at equilibrium. e. Both A and C.

Formula used : Molarity = moles /volume Equilibrium constant = [products]/[reactants]

1. In an experiment, 0.30 mol H2 and 0.30 mol I2 are mixed in a 1.00-L container, and the reaction forms HI. If Ke = 49. for this reaction, what is the equilibrium concentration of HI? H2(g) + I2(g)= = 2HI(g) 2. 2. Which of the following is true for a system whose equilibrium constant is much smaller than one? a. The reaction mixture contains mostly reactants at equilibrium. b. The reaction mixture contains mostly products at equilibrium. c. The rate of reaction is very slow. d. The moles of reactants and products are relatively similar at equilibrium. e. Both A and C.

1. In an experiment, 0.30 mol H2 and 0.30 mol I2 are mixed in a 1.00-L container, and the reaction forms HI. If Ke = 49. for this reaction, what is the equilibrium concentration of HI? H2(g) + I2(g)= = 2HI(g) 2. 2. Which of the following is true for a system whose equilibrium constant is much smaller than one? a. The reaction mixture contains mostly reactants at equilibrium. b. The reaction mixture contains mostly products at equilibrium. c. The rate of reaction is very slow. d. The moles of reactants and products are relatively similar at equilibrium. e. Both A and C.

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...

See similar textbooks

Similar questions

Phosphorus pentachloride decomposes according to the chemical equation Ke = 1.80 at 250 °C PC15 (g) ⇒ PC13(g) + Cl₂(g) A 0.3606 mol sample of PC15 (g) is injected into an empty 3.95 L reaction vessel held at 250 °C. Calculate the concentrations of PC15 (g) and PC13 (g) at equilibrium. [PCI,] = [PC1₂] = M M
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of sulfur dioxide gas and 0.67 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.80 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P 0 x10
Consider the equilibrium reaction: 2SO2(g) + O2(g)---->2SO3(g). You place 1.00 mol/L each of SO2 and O2 in a flask and find that at equilibrium the concentration of SO2 is 0.075 mol/L. What is the equilibrium constant for the reaction of SO2 and O2?
6.
When 3.00 mol of A and 1.00 mol of B are mixed in a 1.00 L vessel, the following reaction takes place: A(g) + B(g) →2 C(g). The equilibrium mixture contains 0.50 mol of C. What is the value of the equilibrium constant for the reaction? 0.24 8.3 O 0.20 0.12
Calculating an equilibrium constant from a partial equilibrium composition Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 35. mol of methane gas and 16. mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 43. mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] с x10 X Ś ? olo 18 Ar
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 75.0 L tank with 4.3 mol of sulfur dioxide gas and 7.2 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 3.0 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. olo K = х10 Ar G Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ......................................... ............................... ..............
Consider the following reaction:2NOBr(g) 2NO(g) + Br2(g)If 0.779 moles of NOBr(g), 0.610 moles of NO, and 0.345 moles of Br2 are at equilibrium in a 11.2 L container at 371 K, the value of the equilibrium constant, Kc,
In a particular experiment, it was found that when O,(g) and CO(g) were mixed and allowed to react according to the equation 2Co(g) + O2(3) = 2CO2(3) the O2 concentration had decreased by 0.062 mol Lwhen the reaction reached equilibrium. How had the concentrations of CO and CO2 changed? [CO] decrease = i mol/L [CO2] increase = mol/L
Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 1.64×10-3 moles of COCl2(g), 0.398 moles of CO, and 0.360 moles of Cl2 are at equilibrium in a 18.2 L container at 843 K, the value of the equilibrium constant, Kc, is .
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 × 10³ at a certain temperature. If the equilibrium concentrations of H₂ and F₂ are both 0.0021 M, determine the concentration of HF at equilibrium. H₂(g) + F₂(g) ⇌ 2 HF(g) Kc = [x]2 / [0.0021] [0.0021] = 2.1x103 [HF]eq =
The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Ke? Cl₂(g) + H₂O(g) = 2 HCl(g) + O₂(g) K = 7.52 x 10-² 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) K = ? OK=177 K = 0.150 OK-5.66 x 10-3 OK 13.3 3 pts ) K = 3.65