MISSED THIS? Read Section 16.6 (Pages 696 - 699).Consider the following reaction:Part ACO (g) + 2 H2 (g)CH;OH (g)An equilibrium mixture of this reaction at a certain temperaturewas found to have [CO] = 0.115 M, H2] = 0.118 M, and[CHOH — 0.190 М.What is the value of the equilibrium constant (K.) at this temperature?Express your answer numerically to three signficant figures.• View Available Hint(s)K. =SubmitProvide Feedback

The equilibrium constant is defined as the ratio of the product of active masses of the products to…

MISSED THIS? Read Section 16.6 (Pages 696 - 699). Consider the following reaction: Part A CO (g) + 2 H2 (g) = CH3OH (g) An equilibrium mixture of this reaction at a certain temperature was found to have CO = 0.115 M, H2] = 0.118 M, and [CHОН- 0.190 М. What is the value of the equilibrium constant (K.) at this temperature? Express your answer numerically to three significant figures. > View Available Hint(s) Πνα ΑΣφ K. = Submit

MISSED THIS? Read Section 16.6 (Pages 696 - 699). Consider the following reaction: Part A CO (g) + 2 H2 (g) = CH3OH (g) An equilibrium mixture of this reaction at a certain temperature was found to have CO = 0.115 M, H2] = 0.118 M, and [CHОН- 0.190 М. What is the value of the equilibrium constant (K.) at this temperature? Express your answer numerically to three significant figures. > View Available Hint(s) Πνα ΑΣφ K. = Submit

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...

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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?