At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) + I½(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2] = 0.447 M, [IL] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] = M [H2) = M %3D M
At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) + I½(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2] = 0.447 M, [IL] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] = M [H2) = M %3D M
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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![General Chemistry 4th Edition
McQuarrie • Rock • Gallogly
University Science Books
presented by Macmillan Learning
At 500 °C, hydrogen iodide decomposes according to
2 HI(g) = H2(g) + I2(g)
For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium:
[H2] = 0.447 M, [I] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction
vessel, what are the equilibrium concentrations after the new equilibrium has been reached?
[HI] =
M
[H2] =
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc3642bbe-9bdc-4a17-a1cb-4f4ee175bfec%2F13f79692-2e11-4fdd-80da-55a9be7ef60f%2F4isud3r_processed.png&w=3840&q=75)
Transcribed Image Text:General Chemistry 4th Edition
McQuarrie • Rock • Gallogly
University Science Books
presented by Macmillan Learning
At 500 °C, hydrogen iodide decomposes according to
2 HI(g) = H2(g) + I2(g)
For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium:
[H2] = 0.447 M, [I] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction
vessel, what are the equilibrium concentrations after the new equilibrium has been reached?
[HI] =
M
[H2] =
M
M
Transcribed Image Text:A student is studying the iron(III)–thiocyanate equilibrium by mixing equal amounts of 0.10 M Fe(NO3)3 and 0.10 M KSCN,
along with some distilled water, into three separate containers. Then, to each container, he mixes in one of the reagents
that follows.
Determine how the equilibrium will be affected by the addition of each reagent, then fill in the statements accordingly.
Fetaq) + SCN (aq) = Fe(SCN)2taq)
Adding 0.10 M Fe(NO3)3 will shift the equilibrium
Adding 0.10 M KSCN will shift the equilibrium
Adding 0.10 M NaOH will shift the equilibrium
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