MASTERING CHEMISTRY:THE CENTRAL SCIENCE
13th Edition
ISBN: 9781269712538
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 23, Problem 2E
Practice Exercise 1
For the reaction
4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6H2O(g) ΔH° = - 90KJ
Which of the following changes will shift the equilibrium to the right, toward the formation of more products?
- Adding more water vapor
- Increasing the temperature
- Increasing the volume of the reaction vessel
- Removing O2(g)
- Adding 1 atm of Ne(g) to the reaction vessel.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Practice Exercise At 1280°C the equilibrium constant (K) for the reaction
Br2(g) 2Br(g)
is 1.1 x 10 . If the initial concentrations are [Br2]
102 M, calculate the concentrations of these species at equilibrium.
6.3 x 10 2 M and [Br]
= 1.2 X
!!
temperature.
Practice Exercise At 1280°C the equilibrium constant (K) for the reaction
Br2(g) 2Br(g)
is 1,1 x 10, If the initial concentrations are [Br2] = 6.3 X 102 M and [Br] = 1.2 x
10 M, calculate the concentrations of these species at equilibrium.
%3D
QUESTION 18
Dinitrogen tetroxide partially decomposes according to the following equilibrium:
N204 (g)
2NO2 (g)
A 1.000-L flask is filled with 0.73 mol of N204. At equilibrium, 0.31 mol of N2O4 remains. Determine the equilibrium constant K for this reaction.
Express your answer in decimal notation to 2 decimal places.
Chapter 23 Solutions
MASTERING CHEMISTRY:THE CENTRAL SCIENCE
Ch. 23.2 - Prob. 23.1.1PECh. 23.2 - Prob. 23.1.2PECh. 23.2 - Prob. 23.2.1PECh. 23.2 - Prob. 23.2.2PECh. 23.4 - The following mechanism has been proposed for the...Ch. 23.4 - Prob. 23.3.2PECh. 23.4 - Prob. 23.4.1PECh. 23.4 - Platinum nanoparticles of diameter ~2 nm are...Ch. 23.4 - 14.114 One of the many remarkable enzymes in the...Ch. 23.4 - 14.115N Suppose that, in the absence of catalyst,...
Ch. 23.5 - Prob. 23.6.1PECh. 23.5 - Dinitrogen pentoxide (N2O5) decomposes in...Ch. 23.6 - The reaction between ethyl iodide and hydroxide...Ch. 23.6 - Prob. 23.7.2PECh. 23.6 - Prob. 23.8.1PECh. 23.6 - Prob. 23.8.2PECh. 23 - Prob. 1DECh. 23 - Practice Exercise 1
If 8.0 g of NH4HS(s)...Ch. 23 - Practice Exercise 1 For the reaction 4 NH3(g) + 5...Ch. 23 - Prob. 3ECh. 23 - Prob. 4ECh. 23 - Phosphorus trichloride gas and chlorine gas react...Ch. 23 - Prob. 6ECh. 23 - Prob. 7ECh. 23 - 15.70 True or false: When the temperature of an...Ch. 23 - Prob. 9ECh. 23 - Prob. 10ECh. 23 - Prob. 11ECh. 23 - Prob. 12ECh. 23 - Prob. 13ECh. 23 - Prob. 14ECh. 23 - Prob. 15ECh. 23 - Practice Exercise 2 For the reaction H2 (g) + I2...Ch. 23 - Prob. 17ECh. 23 - Prob. 18ECh. 23 - Prob. 19ECh. 23 - Practice Exercise 1
A mixture of gaseous sulfur...Ch. 23 - Prob. 21ECh. 23 - Prob. 22ECh. 23 - Practice Exercise 2
The gaseous compound BrCl...Ch. 23 - Prob. 24ECh. 23 - Practice Exercise 2 At 1000 k, the value of Kp for...Ch. 23 - Prob. 26ECh. 23 - Prob. 27ECh. 23 - Practice Exercise 1 For the equilibrium Br2(g) +...Ch. 23 - Prob. 29ECh. 23 - Prob. 30ECh. 23 - Prob. 31ECh. 23 - Prob. 32ECh. 23 - Prob. 33ECh. 23 - Prob. 34ECh. 23 - Prob. 35ECh. 23 - 15.6 Ethene (C2H4) reacts with healogens (X2) by...Ch. 23 - When lead(IV) oxide is heated above 300 O C, it...Ch. 23 - Prob. 38ECh. 23 - The reactin A2(g) + B(g) + A(g) + AB(g) has an...Ch. 23 - The following graph represents the yield of the...Ch. 23 - Suppose that the gas-phase reactions A B and B A...Ch. 23 - Prob. 42ECh. 23 - Prob. 43ECh. 23 - Prob. 44ECh. 23 - Prob. 45ECh. 23 - Prob. 46ECh. 23 - Prob. 47ECh. 23 - Prob. 48ECh. 23 - Prob. 49ECh. 23 - Prob. 50ECh. 23 - Prob. 51ECh. 23 - Prob. 52ECh. 23 - Prob. 53ECh. 23 - Prob. 54ECh. 23 - Prob. 55ECh. 23 - Prob. 56ECh. 23 - Prob. 57ECh. 23 - Prob. 58ECh. 23 - For each of the following metals, write the...Ch. 23 - Prob. 60ECh. 23 - Prob. 61ECh. 23 - Prob. 62ECh. 23 - Prob. 63ECh. 23 - Prob. 64ECh. 23 - Prob. 65AECh. 23 - Prob. 66AECh. 23 - Prob. 67AECh. 23 - Prob. 68AECh. 23 - Prob. 69AECh. 23 - Prob. 70AECh. 23 - Prob. 71AECh. 23 - Prob. 72AECh. 23 - Prob. 73AECh. 23 - Prob. 74AECh. 23 - Prob. 75AECh. 23 - Prob. 76AECh. 23 - Prob. 77AECh. 23 - Prob. 78AECh. 23 - Prob. 79AECh. 23 - Prob. 80AECh. 23 - Prob. 81AECh. 23 - Prob. 82AECh. 23 - Prob. 83AECh. 23 - Prob. 84AECh. 23 - Prob. 85AECh. 23 - Prob. 86AECh. 23 - Prob. 87AECh. 23 - Prob. 88AECh. 23 - Prob. 89AECh. 23 - Prob. 90IECh. 23 - Prob. 91IECh. 23 - Prob. 92IECh. 23 - Prob. 93IECh. 23 - Prob. 94IECh. 23 - Prob. 95IECh. 23 - Prob. 96IECh. 23 - Prob. 97IECh. 23 - Prob. 98IECh. 23 - Prob. 99IECh. 23 - Prob. 100IECh. 23 - Prob. 101IE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- l Verizon ? 1:11 AM 77% 4 Question 4 of 7 Submit Consider the following reaction at equilibrium CO(g) + H20(g) =CO2(g) + H2(g) If CO(g) is removed, in which direction will the equilibrium shift? A) reactants B) products C) no change Tap here or pull up for additional resourcesarrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forwardissue 13Balance the reaction below and write the expression for the equilibrium constant. NO(g) + Cl2(g) ⇌ NOCl(g)I found as a balanced equation: 2NO(g) + Cl2(g) ⇌ 2NOCl(g) and as Kc= 2.5 x 103.Is it correct ?arrow_forward
- 13 ut of Toluene, C₂Hs(9), is an important organic solvent and can be produced as represented by the following equilibrium equation. CH₁4(g) + energy C7Hs (g) + 3H₂(g) The equilibrium expression for this reaction equation is Select one: Kc = Kc = Kc = Kc = [C7Hs (g)]³[H₂(g)] [C7H14(g)] [C7H14(g)] [C7H8(g)]³[H₂(g)] [C7H8(g)][H₂(g)} [C7H₁4(g)] [C7H14(g)] [C7H8(g)][H₂(g)]³arrow_forwardQuestion 2 of 4 Submit For the reaction: 2 A (g) + B (s) =2 C (s) + D (g) At 298 K in a 10.0 L vessel, the equilibrium values are as follows: 0.721 atm of A, 4.18 mol of B, 6.25 mol of C, and 5.06 atm of D. What is the value of the equilibrium constant? 8.06 1 2 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources 3. LOarrow_forwardQUESTION 32 ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant for the following system is 0.0075 at 373 K. 2 503(g) = 2 50₂(g) + O₂(g) The initial concentrations of SO3, SO₂, and O₂ are 3.0 M, 2.0 M, and 1.0 M. Complete the ICE table to show the changes and equilibrium concentrations using the values from the following list. Provide your answer below: I C E [SO3] [SO₂] [0₂]arrow_forward
- Which of the following statements is (are) true? (Select all that apply.) If equilibrium constants for the chemical reaction N2(g) + O2(g) : = 2 NO(g) are K, = 1.1 x 103 and 3.6 x 103 at 2,200 K and 2,500 K, respectively, then the reaction is exothermic. If Q < K then the reactant concentrations will be decrease as the reaction proceeds to equilibrium. Concentration of the products equals the concentrations of the reactants. If the reaction, C(s) + 2H2(g) = CH4(g) is at equilibrium, adding solid carbon will cause the reaction to shift in the forward direction. None of these statements are true. O At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.arrow_forwardissue 6Choose the equilibrium in which the products are favored by a drop in pressure and the reactants favored by a drop in temperature.a) N2(g) + 3 H2(g) ⇔ 2 NH3(g) + 92.3 kJb) H2(g) + I2(g) + 51.8 kJ ⇔ 2 HI(g)c) PCl3(g) + Cl2(g) ⇔ PCl5(g) ΔH = -84.2 kJd) 2 NO2(g) ⇔ 2 NO(g) + O2(g) ΔH = +54 kJarrow_forward(Incorrect) For the reaction 2A(g) + B(s) C() + 2D(g) at 700 °C, Kc = 0.00577. Calculate the number of moles of D present at equilibrium if a mixture of 6.03 moles of C and 6.03 moles of D is heated to 700 °C in a 7.61-L container. 0.0074 mol (Your answer) 0.430 mol (Correct answer) 5.60 mol 0.056 molarrow_forward
- 5 Question 26 For the equilibrium system below. CH,(g) + H2O (g) CO (g) + 3 H₂ (9) which modification would result in a shift toward reactants? decreasing partial pressure of CO increasing temperature increasing partial pressure of CH4 decreasing system volume ΔΗ° = -206 kJarrow_forwardFor the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210 At 298 K in a 10.0 L vessel, the known equilibrium values are as follows: 0.016 atm of A, 0.22 mol of B, and 10.5 mol of C. What is the equilibrium partial pressure of D? Answer ____ atmarrow_forwardMa Question 14 At 25°C, the equilibrium constant, Kc, for the following reaction is 0.045. 2E(g) F(g) + G(g) A mixture of 0.800 moles of F and 1.200 mole of G in a 2.0-L container is allowed to come to equilibrium. What is the equilibrium concentration of E in molar? Please report 3 decimal places, without units. Question 15 Which pair of substances willarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY