Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP
Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP
14th Edition
ISBN: 9780134661483
Author: Edward L Waterman
Publisher: PEARSON
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Chapter 15, Problem 1DE

(a)

Interpretation Introduction

To determine:

The gas or gases whose concentration can be monitored by using a spectrophotometer.

(a)

Expert Solution
Check Mark

Answer to Problem 1DE

Solution:

The concentration of iodine gas can be monitored with the spectrometer.

Explanation of Solution

The spectrometer is a device which splits light into the array of separate colors which is shown as a spectrum on the spectrometer.

The gases which absorb in the visible region can only be monitored by the spectrometer. Since iodine gas lies in the visible region and gives violet color so, the concentration of iodine gas can be monitored with the spectrometer.

(b)

Interpretation Introduction

To determine:

The way to determine the extinction coefficient for the given substance.

(b)

Expert Solution
Check Mark

Answer to Problem 1DE

Solution:

The extinction coefficient is calculated by the slope of absorbance versus concentration graph.

Explanation of Solution



The absorbance of the given solution is calculated by using the formula,

    A=εbc

Where,

  • A is the absorbance of the solution.
  • ε is the extinction coefficient.
  • b is the path length of the solution.
  • c is the concentration of the solution.

Therefore, the plot of A versus c gives slope equals to the bε . The path of the solution is known and hence, the extinction coefficient can be calculated.

(c)

Interpretation Introduction

To determine:
The experiment to calculate the equilibrium constant at 600K .

(c)

Expert Solution
Check Mark

Answer to Problem 1DE

Solution:

The sample containing an equal concentration of hydrogen and iodine is used to determine the equilibrium constant of the reaction.

Explanation of Solution



The balanced chemical equation for the given reaction is,

    H2(g)+I2(g)2HI(g)

The equilibrium constant of the given reaction is calculated by using the formula,

    Kc=[HI]2[H2][I2]

The experiment that can be performed to calculate the equilibrium constant for the given reaction is to determine the absorbance of the sample solution containing equal concentrations of hydrogen and iodine which can be used to calculate the concentration of given solution.

(d)

Interpretation Introduction

To determine:

The enthalpy of the given reaction by using the bond enthalpy values.

(d)

Expert Solution
Check Mark

Answer to Problem 1DE

Solution:
The enthalpy of the given reaction is 11kJ/mol .

Explanation of Solution



The balanced chemical equation for the given reaction is:

    H2(g)+I2(g)2HI(g)

The enthalpy of the given reaction is calculated by using the formula,

    ΔH=E BondsbrokenE Bondsformed=E(HH)+E(II)2E(HI)

Substitute the values of E(HH) , E(II) and E(HI) in the above equation.

    ΔH=436kJ/mol+151kJ/mol2×299kJ/mol=11kJ/mol

(e)

Interpretation Introduction

To determine:
If the value of Kc at 600K is smaller or larger than that of the value at 300K .

(e)

Expert Solution
Check Mark

Answer to Problem 1DE

Solution:
The value of the equilibrium constant at 300K is larger than the value at 600K .

Explanation of Solution

The value of enthalpy of the reaction is negative as the answer in part (d) which means the energy is released in the given reaction. Therefore, the increase in temperature results in the shifting of equilibrium in backward direction. Thus, the value of equilibrium constant declined by increasing temperature.

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Chapter 15 Solutions

Test Prep Series for AP Chemistry for Chemistry: The Central Science 14th ed AP

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
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