General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
5th Edition
ISBN: 9780321967466
Author: Karen C. Timberlake
Publisher: PEARSON
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Chapter 10, Problem 10.50AQAP
Consider the reaction: (10.3)
a Write the equilibrium constant expression
b What is the numerical value of K. for the reaction it the concentrations at equilibrium are
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8.) Consider the following equilibrated system: 2NO2(g)=2NO(g) + O2(g). If the Kc value
is 0.918, find the equilibrium concentration of the O2 gas if the NO2 concentration is 0.520
M and the [NO] is 0.300 M at equilibrium. (2.76 M)
At high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.
Which change causes the equilibrium to shift to the product side?
2 CO) + O2(2) 2 CO2(2) AH= -
(3)0)
283.3kJ
(3)2)
(3)2)
ORemoving oxygen
O Increasing the temperature
O Adding carbon dioxide
Removing carbon monoxide
Decreasing the volume
Chapter 10 Solutions
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Ch. 10.1 - What is meant by the rate of a reaction? Why does...Ch. 10.1 - How does a catalyst affect the activation energy?...Ch. 10.1 - Prob. 10.3QAPCh. 10.1 - Prob. 10.4QAPCh. 10.1 - Prob. 10.5QAPCh. 10.1 - Prob. 10.6QAPCh. 10.2 - Prob. 10.7QAPCh. 10.2 - Prob. 10.8QAPCh. 10.2 - Prob. 10.9QAPCh. 10.2 - Prob. 10.10QAP
Ch. 10.2 - Prob. 10.11QAPCh. 10.2 - Prob. 10.12QAPCh. 10.3 - Prob. 10.13QAPCh. 10.3 - Prob. 10.14QAPCh. 10.3 - Prob. 10.15QAPCh. 10.3 - Prob. 10.16QAPCh. 10.3 - Prob. 10.17QAPCh. 10.3 - Prob. 10.18QAPCh. 10.3 - Prob. 10.19QAPCh. 10.3 - Prob. 10.20QAPCh. 10.4 - Prob. 10.21QAPCh. 10.4 - Prob. 10.22QAPCh. 10.4 - Prob. 10.23QAPCh. 10.4 - Prob. 10.24QAPCh. 10.4 - Prob. 10.25QAPCh. 10.4 - Prob. 10.26QAPCh. 10.4 - Prob. 10.27QAPCh. 10.4 - The Kc for the following reaction at 225C is...Ch. 10.5 - Prob. 10.29QAPCh. 10.5 - Ammonia is produced by reacting nitrogen gas and...Ch. 10.5 - Prob. 10.31QAPCh. 10.5 - Prob. 10.32QAPCh. 10.5 - Prob. 10.33QAPCh. 10.5 - Prob. 10.34QAPCh. 10.5 - Prob. 10.35QAPCh. 10.5 - Prob. 10.36QAPCh. 10.5 - Prob. 10.37QAPCh. 10.5 - Prob. 10.38QAPCh. 10 - Prob. 10.39UTCCh. 10 - Prob. 10.40UTCCh. 10 - Prob. 10.41UTCCh. 10 - Prob. 10.42UTCCh. 10 - Prob. 10.43UTCCh. 10 - Prob. 10.44UTCCh. 10 - Prob. 10.45AQAPCh. 10 - For each of the following changes at equilibrium,...Ch. 10 - Prob. 10.47AQAPCh. 10 - Prob. 10.48AQAPCh. 10 - Consider the reaction: (10.3) 2NH3gN2g+3H2g a...Ch. 10 - Consider the reaction: (10.3) 2SO2g+O2g2SO3g a...Ch. 10 - Prob. 10.51AQAPCh. 10 - Prob. 10.52AQAPCh. 10 - According to Le Châtelier’s principle, does the...Ch. 10 - Prob. 10.54AQAPCh. 10 - Prob. 10.55AQAPCh. 10 - Prob. 10.56AQAPCh. 10 - Prob. 10.57CQCh. 10 - Prob. 10.58CQCh. 10 - Prob. 10.59CQCh. 10 - Prob. 10.60CQCh. 10 - Prob. 10.61CQCh. 10 - Prob. 10.62CQCh. 10 - Prob. 10.63CQCh. 10 - Indicate if you would increase or decrease the...
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- 10. 1) Please choose the corect expression and circle it. Le chatelier's Principle Summarized Below Change Concentration Pressure Volume Shifts Equilibrium Change Equilibrium Constant yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no Temperature Catalyst ii) 250:(g)+0:(3)2SO:(g) The position of equilibrium moves to the right/left if the concentration of SO; is increased. Co.(g) CO(g)+O( If we increase the pressure of COg), the system will shift towards the reactants/products because it has a fewer/more number of moles of gas. CIHH:0 HO'+Cl+Heat If we decrease the temperature, the reaction will proceed towards the reactants/products because the system must regenerate/used the heat that was lost/gain. iii) Will the equilibrium in reactionarrow_forward12 (9) H₂ (9) In which direction will equilibrium shift if H2 gas is added to the system? + HI is removed as soon as formed? 2HI (g)arrow_forwardPredict the equilibrium partial pressure of NO in the reaction described below (for which Kp = 60.6 at the reaction temperature) by constructing an equilibrium expression for Qp, constructing an ICE table, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure. Complete Parts 1-4 before submitting your answer. (0.20) 3 NEXT > An initial mixture of 0.20 atm of every species is allowed to react. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qp. (0.40) 0.40 (0.40) (0.20)² 0.040 Qp = (0.20) 2 NOBr(g) = 2 NO(g) + Br₂(g) (0.40)² 0.020 2 (0.40) (x) (0.20) = (0.40) 4 (2x) (0) (2x)² RESET (0.20) 0.20arrow_forward
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- 6.56 Use each expression for the equilibrium constant to write a chemical equation. 88.D [AB,]² [A,][B,]² [A,B,] illupe 1ot a6. K= w a. K = e erl) wollot [A]°[B]³ %3Barrow_forward1.4 4 (a) Calculate the value of Kc for the reaction: PC15 (8) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PC15 (g): is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PC15 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (i) Increasing temperature (ii) Lowering the concentration of chlorine (C1₂) (iii) Addition of a catalystarrow_forward9.28 When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s) + H₂O(g) + Heat CO(g) + H₂(g) In which direction will the equilibrium shift (right or left) if the following changes occur to the reaction at equilibrium? a. add heat b. lower temperature c. remove CO d. add H₂Oarrow_forward
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