EBK CHEMISTRY:CENTRAL SCIENCE
14th Edition
ISBN: 9780134554570
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15.5, Problem 15.8.1PE
Practice Exercise 1
In Section 15.1, we discussed the equilibrium between N2O4(g) and NO2(g). Lets return to that equation in a quantitative example. When 9.2 g of frozen N2O4 is added to a 0.50 L reaction vessel that is heated to 400 k and allowed to come to equilibrium, the concentration of N2O4 is determined to be 0.057 M. Given this information, what is the value of Kc for the reaction N2O4(g) ⇌ 2NO2(g) at 400k?
- 0.23
- 0.36
- 0.31
- 1.4
- 2.5
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Carbon monoxide and hydrogen react according to the following equation: CO (g) + H2 (g) CH4 (g) + H2O (g)
When 1.00 mol of CO and 3.00 moles of H2 are placed in a 10.0 L container at 927 ° C (1200 K) and allowed to reach equilibrium, the mixture is found to have 0.363 moles of H2O
What is the molar composition (that is, how many moles) of H2 are present in the equilibrium mixture? Answer:
Which of the following does not represent a homogeneous equilibrium? [Select all that apply]
Group of answer choices
N2O4 (g) ⇄ 2 NO2 (g)
N2 (g) + 3 H2 (g) ⇄ 2 NH3 (g)
CaCO3 (s) ⇄ CaO (s) + CO2 (g)
H2 (g) + I2 (g) ⇄ 2 HI (g)
Co (s) + 2H+ (aq) ⇄ Co2+ (aq) + H2 (g)
2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)
You have 0.4 moles C2H2 and 0.2 moles O2 present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process?
Question 5 options:
Conc.
C2H4
O2
CO2
H2O
Initial
0.4
0.2
0
0
Change
-x
-x
+x
+x
Equil.
0.4-x
0.2-x
x
x
Conc.
C2H4
O2
CO2
H2O
Initial
0.08
0.04
0
0
Change
-2x
-5x
+4x
+2x
Equil.
0.08-2x
0.04-5x
4x
2x
Conc.
C2H4
O2
CO2
H2O
Initial
0.4
0.2
0
0
Change
-2x
-5x
+4x
+2x
Equil.
0.4-2x
0.2-5x
4x
2x
Conc.
C2H4
O2
CO2
H2O
Initial
0.08
0.04
0
0
Change
-20x
-20x
+20x
+20x
Equil.
0.08-20x
0.04-20x
20x
20x
Chapter 15 Solutions
EBK CHEMISTRY:CENTRAL SCIENCE
Ch. 15.2 - Prob. 15.1.1PECh. 15.2 - Prob. 15.1.2PECh. 15.2 - Prob. 15.2.1PECh. 15.2 - Prob. 15.2.2PECh. 15.3 - Prob. 15.3.1PECh. 15.3 - Practice Exercise 2 For the reaction H2 (g) + I2...Ch. 15.3 - Prob. 15.4.1PECh. 15.3 - Prob. 15.4.2PECh. 15.4 - Prob. 15.5.1PECh. 15.4 - Prob. 15.5.2PE
Ch. 15.4 - Practice Exercise 1
If 8.0 g of NH4HS(s)...Ch. 15.4 - Prob. 15.6.2PECh. 15.5 - Practice Exercise 1
A mixture of gaseous sulfur...Ch. 15.5 - Prob. 15.7.2PECh. 15.5 - Practice Exercise 1 In Section 15.1, we discussed...Ch. 15.5 - Practice Exercise 2
The gaseous compound BrCl...Ch. 15.6 - Prob. 15.9.1PECh. 15.6 - Practice Exercise 2 At 1000 k, the value of Kp for...Ch. 15.6 - Prob. 15.10.1PECh. 15.6 - Prob. 15.10.2PECh. 15.6 - Practice Exercise 1 For the equilibrium Br2(g) +...Ch. 15.6 - Prob. 15.11.2PECh. 15.7 - Practice Exercise 1 For the reaction 4 NH3(g) + 5...Ch. 15.7 - Prob. 15.12.2PECh. 15 - Prob. 1DECh. 15 - Based on the following energy profile, predict...Ch. 15 - 15.2 The following diagrams represent a...Ch. 15 - Prob. 3ECh. 15 - Prob. 4ECh. 15 - Prob. 5ECh. 15 - 15.6 Ethene (C2H4) reacts with healogens (X2) by...Ch. 15 - When lead(IV) oxide is heated above 300 O C, it...Ch. 15 - Prob. 8ECh. 15 - The reactin A2(g) + B(g) + A(g) + AB(g) has an...Ch. 15 - Prob. 10ECh. 15 - Prob. 11ECh. 15 - The following graph represents the yield of the...Ch. 15 - Suppose that the gas-phase reactions A B and B A...Ch. 15 - Prob. 14ECh. 15 - Prob. 15ECh. 15 - Write the expression for KC for the following...Ch. 15 - When the following reaction come to equilibrium,...Ch. 15 - Prob. 18ECh. 15 - Prob. 19ECh. 15 - Prob. 20ECh. 15 - If Kc = 0.042 for PC13(g) + C12 (g) PC15 (g) at...Ch. 15 - Prob. 22ECh. 15 - 15.23 The equilibrium constant for the...Ch. 15 - Prob. 24ECh. 15 - Prob. 25ECh. 15 - Prob. 26ECh. 15 - The following equilibria were attained at 823 K:...Ch. 15 - Consider the equilibrium N2(g) + O2(g) + Br2(g) 2...Ch. 15 - Mercury(I) oxide decomposes into elemental mercury...Ch. 15 - Prob. 30ECh. 15 - Prob. 31ECh. 15 - Prob. 32ECh. 15 - Prob. 33ECh. 15 - Phosphorus trichloride gas and chlorine gas react...Ch. 15 - A mixture of 0.10 mol of NO, 0.050 mol of H2, and...Ch. 15 - Prob. 36ECh. 15 - A mixture of 0.2000 mol of CO2, 0.1000 mol of H2,...Ch. 15 - 15.38 A flask is charged with 1.500 atm of N2O4(g)...Ch. 15 - Prob. 39ECh. 15 - Prob. 40ECh. 15 - a. If QC KC, in which direction will a reaction...Ch. 15 - Prob. 42ECh. 15 - At 100 OC , the equilibrium constant for the...Ch. 15 - 15.44 As shown in Table 15.2, KP for the...Ch. 15 - At 100 C, K = 0.078 for the reaction SO2Cl2 (g) ...Ch. 15 - Prob. 46ECh. 15 - Prob. 47ECh. 15 - Prob. 48ECh. 15 - At 800 k, the equilibrium constant for I2 (g) ...Ch. 15 - Prob. 50ECh. 15 - At 2000 OC, the equilibrium constant for the...Ch. 15 - For the equilibrium Br2 (g) + Cl2 (g) 2BrCl(g) At...Ch. 15 - At 373 k, Kp = 0.416 for the equilibrium 2NOBr (g)...Ch. 15 - At 218 oC, KC= 1.2 X 10-4 for the equilibrium NH4...Ch. 15 - Prob. 55ECh. 15 - At 80 oC, K =1.87 X 10-3 for the reaction PH3 BCl3...Ch. 15 - Prob. 57ECh. 15 - Prob. 58ECh. 15 - Prob. 59ECh. 15 - Prob. 60ECh. 15 - Consider the following equilibrium for which H<0...Ch. 15 - Prob. 62ECh. 15 - 15.63 How do the following changes affect the...Ch. 15 - Prob. 64ECh. 15 - Consider the following equilibrium between oxides...Ch. 15 - Prob. 66ECh. 15 - Ozone, O3, decomposes to molecular oxygen in the...Ch. 15 - Prob. 68ECh. 15 - Prob. 69ECh. 15 - 15.70 True or false: When the temperature of an...Ch. 15 - Prob. 71AECh. 15 - Prob. 72AECh. 15 - 15.73 A mixture of CH4 and H2O is passed over a...Ch. 15 - Prob. 74AECh. 15 - Prob. 75AECh. 15 - Prob. 76AECh. 15 - Prob. 77AECh. 15 - Prob. 78AECh. 15 - Prob. 79AECh. 15 - For the equilibrium PH3BCI3 (s) PH3 (g) + BCI3...Ch. 15 - Prob. 81AECh. 15 - Prob. 82AECh. 15 - Prob. 83AECh. 15 - At 900 o C, Kc = 0.0108 for the reaction CaCO3(g) ...Ch. 15 - Prob. 85AECh. 15 - The equilibrium constant Kc for C(s) +CO2 2CO(g)...Ch. 15 - Prob. 87AECh. 15 - Le Chatelier noted that many industrial processes...Ch. 15 - Prob. 89AECh. 15 - Prob. 90AECh. 15 - [15.91] An equilibrium mixture of H2, I2, and HI...Ch. 15 - Consider the hypothetical reaction A(g) + 2B(g) 2...Ch. 15 - Prob. 93AECh. 15 - Prob. 94AECh. 15 - Prob. 95IECh. 15 - The following equilibria were measured at 823 K:...Ch. 15 - Prob. 97IECh. 15 - Prob. 98IECh. 15 - At 800 K, the equilibrium constant for the...Ch. 15 - Prob. 100IECh. 15 - Prob. 101IECh. 15 - Prob. 102IE
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
- Consider the following equilibrium: 2HF(g)⇌H2(g)+F2(g) At equilibrium, the concentration of hydrogen fluoride gas, hydrogen gas, and fluorine gas are 2.04 mol/L, 2.47 mol/L, and 1.89 mol/L. What is the value of the equilibrium constant? Answer to 3 decimal places.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_forwardSuppose the reaction A ⇀↽ B has an equilibrium constant of 1.0. The initial concentration of A is 0.63 M and the initial concentration of B is 0.28 M. What is the equilibrium concentration of A? Answer in units of M.arrow_forward
- ASK YOUR TEACHER PRACTICE ANOTHER Determine the value of the equilibrium constant for the following reaction occurring at SATP. 2 NH3(g) N2(g) + 3 H2(g) ΔG° = 32.7 kJ/molarrow_forwardThe following reaction is at equilibrium: CH4 + 2 Cl2 ⇌ CH2Cl2 + 2 HCl If the partial pressures are: CH4 = 0.250 bar, Cl2 = 0.150 bar, and CH2Cl2 = 0.175 bar at equilibrium, what is the partial pressure of HCl at equilibrium if the K is 2.30? Question options: 0.356 0.272 0.007 0.391arrow_forward< Progress:0/9 groups Due Apr 18 at 11:55 PM Use the References to access important values if needed for this question. In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+(aq) is pink and CoCl42-(aq) is blue. ... At Low Temperature the pink color predominates. ... ... At High Temperature the blue color is strong. ... If we represent the equilibrium as:...Co2+(aq) + 4Cl-(aq) CoCl42-(aq)We can conclude that: fill in the blank 1 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. fill in the blank 2 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. fill in the blank 3 3. When the temperature is decreased the equilibrium concentration of Co2+: A. Increases B. Decreases…arrow_forward
- question 13 The reaction Cl2(g) + F2(g) ⇌ 2ClF(g) has Kc = 1.0 ×109 at a certain temperature. If 1.0 mol Cl2 and 1.0 mol F2 are placed in a 1.0 L reaction vessel and allowed to react, then at equilibrium… Question 13 options: The system will contain only Cl2 and F2. [ClF] will be much larger than [Cl2] and [F2]. [ClF] will be nearly equal to [Cl2] and [F2]. [ClF] will be much less than [Cl2] and [F2]. The system will contain only ClF.arrow_forwardStuck on a practice test problem."If AgCl(s) is in equilibrium with dissolved AgCl according to the following equation:AgCl(s) <-> Ag+(aq) + Cl-(aq)If the equilibrium constant for this process is: Kc = -1.8*10-10, what is the Ag+ concentration when AgCl is dissolved in pure water?"A. 1.3*10-5B. 2.8*10-5C. 3.6*10-10D. 9.0*10-11E. 5.5*10-6 The answer key says it is A, but I am unsure of how to get there. Any explanation on where to start would be greatly appreciated!arrow_forwardWhat are the moles of N2 present at equilibrium at 450oC if 1.00 mol N2 and 4.00 mole H2 in a 10.0 L vessel react according to the following equation? The equilibrium constant Kp is 4.29 x10-5. N2 (g) + 3 H2 (g) ⇋ 2 NH3 (g). Please type answer not write by hendarrow_forward
- issue 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_forwardConsider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. A(g)B(g)K=2X(g)2Y(g)K=62C(g)D(g)K=1 Assume that the reactions have reached equilibrium. Match each of these reactions with one of the containers I to IV (each of which has a volume of 1 L). Identify the color of each molecule (for example, is A red or blue?).arrow_forwardWhy is an equilibrium constant unitless? Answer:arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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