QUESTION 1"For the reaction of molecular iodine gas into atomic iodine gas, the equilibrium constant K e is 0.00213958778017127 at 707°C for thefollowing reaction:11 2(g)--2(8)If the initial concentration of I 2(g)is 0.15M, what is the equilibrium concentration of I(g)?"

Kc is the ratio of product of concentration of products raised to their stoichiometric coefficient…

"For the reaction of molecular iodine gas into atomic iodine gas, the equilibrium constant Ke is 0.00213958778017127 at 707°Cc for the following reaction: 11 2(g)--2(g) If the initial concentration of I 2(g)is 0.15M, what is the equilibrium concentration of I(g)?"

"For the reaction of molecular iodine gas into atomic iodine gas, the equilibrium constant Ke is 0.00213958778017127 at 707°Cc for the following reaction: 11 2(g)--2(g) If the initial concentration of I 2(g)is 0.15M, what is the equilibrium concentration of I(g)?"

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 60E: At a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the...

See similar textbooks

Similar questions

Consider the isomerization of butane with an equilibrium constant of K = 2.5. (See Study Question 13.) The system is originally at equilibrium with [butane] = 1.0 M and [isobutane] = 2.5 M. (a) If 0.50 mol/L of isobutane is suddenly added and the system shifts to a new equilibrium position, what is the equilibrium concentration of each gas? (b) If 0.50 mol/L of butane is added to the original equilibrium mixture and the system shifts to a new equilibrium position, what is the equilibrium concentration of each gas?
Nitrosyl bromide, NOBr, dissociates readily at room temperature. NOBr(g) NO(g) + Br2(g) Some NOBr is placed in a flask at 25 C and allowed to dissociate. The total pressure at equilibrium is 190 mm Hg and the compound is found to be 34% dissociated. What is the value of Kp?
question 1: For the following chemical reaction, the equilibrium constant has a value of 1.37 x 10-3. We would expect the concentration of products, at equilibrium, to be __________ the concentration of reactants.
QUESTION 6 The value of the equilibrium constant for the following reaction is 24 at a given temperature: N2(g) + 3H2(g) ⇌ 2NH3(g) If [N2] = 10.0 M, [H2] = 10.0 M, and [NH3] = 10.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium? Since Q = 0.01, the reaction is not at equilibrium, it will shift to the left. It is not possible to tell if the reaction is at equilibrium. Since Q = 1, the reaction is not at equilibrium, it will shift to the left. Since Q = 1, the reaction is not at equilibrium, it will shift to the right. Since Q = 100, the reaction is not at equilibrium, it will shift to the right. Since Q = 100, the reaction is not at equilibrium, it will shift to the left. The reaction is at equilibrium. To reach equilibrium, the value of Keq must change. Since Q = 0.01, the reaction is not at equilibrium, it will shift…
QUESTION 44 In the fictitious reaction below, the equilibrium concentration of A is 0.2024 M, B is 0.7852 M, and A 2B 3 is 0.3058 M. What is the value of the equilbrium constant k c for this reaction? 2 A (aq) + 3 B (aq) <-> A 2B 3 15.42 1.924 2.856 59.82 0.06485
QUESTION#1: TOPIC: Calculating an equilibrium constant from a heterogeneous equilibrium composition Nickel carbonyl decomposes to form nickel and carbon monoxide, like this: NiCO4(g)→Ni(s)+4CO(g) At a certain temperature, a chemist finds that a 2.9 L reaction vessel containing a mixture of nickel carbonyl, nickel, and carbon monoxide at equilibrium has the following composition: compound amount NiCO4 0.792 g Ni 71.9 g CO 1.17 g Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to 2 significant digits. Kc= ? QUESTION#2: TOPIC: Calculating the pH of a strong acid solution A chemist dissolves 185. mg of pure hydroiodic acid in enough water to make up 300. mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. ?
The reaction quotient, Q, for a reaction has a value of 75 while the equilibrium constant, K, has a value of 195. Which of the following statements is accurate? Question 3 options: The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium. The reaction must proceed to the right (towards products) to establish equilibrium. The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium. The reaction must proceed to the left (towards reactants) to establish equilibrium.
Question: In a closed system, a reaction occurs between two gases, A and B, according to the following balanced equation: 2A(g) + 3B(g) ⇌ C(g) + 2D(g) The reaction is initially at equilibrium. If the pressure of gas A is increased while keeping the temperature and the pressure of gas B constant, what will be the effect on the equilibrium position of the reaction? Justify your answe.
Question 13: The reaction attached below has an equilibrium constant of 1.30 at 650 °C. Carbon monoxide and steam both have initial partial pressure of 0.485 atm, while hydrogen and carbon dioxide start with partial pressures of 0.159 atm. Calculate the partial pressure of each gas at equilibrium.
Consider the following equilibrium, established in a 2.0 L flask at 50ºC. CH4(g) + 2H2S(g) CS2(g) + 4H2(g) If the pressure is increased by decreasing the volume of the container, in which direction will the equilibrium shift? Question 7 options: A) To the left. B) The equilibrium will not shift. C) To the right.
QUESTION 13 Consider the following reaction and its equilibrium constant at 100°C: N2O4(g) ⇌ 2NO2(g) Keq = 6.5 If 0.250 mol of each reactant and product is mixed into a 2.0−L container, will the reaction proceed in the forward or reverse direction, or is it already at equilibrium? Since Q = 8, the reaction will proceed in the forward direction because there is too much NO2 and too little N2O4 in the system. The reaction is already at equilibrium. Since Q = 0.125, the reaction will proceed in the forward direction because there is too much N2O4 and too little NO2 in the system. Since Q = 8, the reaction will proceed in the reverse direction because there is too much NO2 and too little N2O4 in the system. Since Q = 0.125, the reaction will proceed in the reverse direction because there is too much N2O4 and too little NO2 in the system.
A)Which of the following changes to the equilibrium system represented above will increase the quantity of HF(g) in the equilibrium mixture? H2(g) + F2(g) ⇄ 2 HF(g) ΔH > 0 I. Adding H2(g) II. Increasing the temperature III. Decreasing the pressure Question 1 options: a I only b III only c I and II only d II and III only e I, II, and III b) The equilibrium constant would be affected by which of the following changes in conditions: Question 2 options: a temperature b changes in concentration c volume changes when a gas is present d changes to the pressure, if a gas is present e temperature and changes in concentration