At 1280°C the equilibrium constant Ke for the reactionBr2(g)=2Br(g)is 1.1 × 103. If the initial concentrations are [Br2] = 0.0400 M and [Br] = 0.0390 M, calculate theconcentrations of these two species at equilibrium.[Br₂leq[Br]eq==MM

Given equilibrium constant Kc=1.1×10−3and initial concentrations[Br2]=0.0400 M[Br]=0.0390 MDrawing…

Answered: At 1280°C the equilibrium constant Ke…

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

Consider the decomposition of nitrosyl bromide into nitrogen monoxide and bromide gas, which has an equilibrium constant Kc = 6.2 x 10-5 when the reaction occurs at a certain temperature. If the initial concentration of nitrosyl bromide is 0.832 M, what will be the equilibrium concentration of nitrogen monoxide gas? 2 BrNO (g) <---> 2 NO (g) + Br2 (g)
Consider the following reaction: 4 NHK + 50.210, 04 NO. + 6H2O) If 1.00 mole of NH, 1.00 mole of O, 1.00 mole of NO, and 1.00 mole of H2O are allowed to react in a 4.00-liter container, at a particular temperature, the equilibrium concentration of NH, was 0.200 mol/Liter. Calculate the equilibrium concentration of all species and the value of the K.
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
The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) = C₂H₂(g) + 3H₂(g) K₂=1. × 10¯¯ P -7 He fills a reaction vessel at this temperature with 11. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. 0 yes no atm x10 Ś
8. Consider the reaction: CO + 3H2(g) ↔ CH4(g) + H2O(g) At 500 K, the equilibrium constant for this reaction is KP = 2.48 × 10^-3. Suppose we fill a 7.50 L flask with the four gases. When the mixture reaches equilibrium, the flask contains 0.521 g CO, 0.521 g H2, and 9.20 g H2O. How many grams of CH4 are present?
For the reaction 2 NO(g) + Cl2 (g) *double arrow here* 2 NOCl (g) at 25 ℃, the equilibrium constant is 10.0. If at equilibrium, [NOCl] = 2.6 M, [NO] = 0.34 M, what is the concentration of chlorine gas?
Enter your answer in the provided box. In an analysis of the following reaction at 100°C, Br2(g) + Cl2(g) = 2BRCI(g) the equilibrium concentrations of the reactants were found to be [Br2] = 4.3 × 10 M and [Cl2] = 7.4 x 10 M. The equilibrium constant is K. = 7.1. Determine the value of [BrCI].
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 6. N,(g) + 2H,0(g) 2 NO(g) + 2 H, (g) K,=7. × 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.7 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H,, using only the tools yes x10 available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.
Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .
The reaction SO,Cl,(g) 2 SO2(g) + Cl,(g) has an equilibrium constant at 100°C of 2.40. Calculate the concentration of SO, that will be present at 100°C in equilibrium with SO2C1, (at a concentration of 3.6 x 10-4 mol L-1) and chlorine (at a concentration of 6.9 × 10-3 mol L¯1).
At a certain temperature, the equilibrium constant, K., is 0.00572 for the reaction Cl,(g) = 2 Cl(g) A. If 2.77 g Cl, is placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl, and Cl? [CI,] = M [CI] = M B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 5.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and Cl? [Cl,] = M [CI] = M C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.0 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and CI? [Cl,] = M [CI] = M

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

At 1280°C the equilibrium constant Ke for the reaction Br2(g)=2Br(g) is 1.1 × 103. If the initial concentrations are [Br2] = 0.0400 M and [Br] = 0.0390 M, calculate the concentrations of these two species at equilibrium. [Br₂leq [Br]eq= = M M