CHEMISTRY >CUSTOM<
14th Edition
ISBN: 9781259137815
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 18.3, Problem 1PPB
Practice Problem
BUILD
Make a qualitative prediction of the sign of
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Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.(a) H2(g)+I2(g)⟶2HI(g) T=400°C Kp=50.0(b) CaCO3(s)⟶CaO(s)+CO2(g) T=900°C Kp=1.04(c) HF(aq)+H2O(l)⟶H3O+(aq)+F−(aq) T=25°C Kp=7.2×10−4(d) AgBr(s)⟶Ag+(aq)+Br−(aq) T=25°C Kp=3.3×10−13
Calculate AG°
reaction spontaneous (yes or no
Answer with 3 sig figs
PC13 (g) + Cl₂(g) →PCI5 (g)
Species
PC|3 (g)
Cl₂(8)
PC15(g)
9
AS°
AH (kJ/mol)
0
-288.0
-374.9
|)?
9
and ΔΗ°
AS (J/mol-K)
311.8
223.1
364.5
for the reaction below at 25 degrees C. Is the
(28)
The standard Gibbs free energy associated with the following reaction is -91.2 kJ:
HCI (g) + NH3 (g) → NH,CI (s)
What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm
and the partial pressure of NH3 (g) is 0.284 atm?
(A)
(B)
-95.1 kl
-90.7 kl
(C)
(D)
(E)
3.93 kJ
noltemol or ni lu bluos noinsou
-79.5 kJ
-87.3 kJ
Chapter 18 Solutions
CHEMISTRY >CUSTOM<
Ch. 18.1 - Practice Problem ATTEMPT
Determine the change in...Ch. 18.1 - Practice Problem BUILD To what fraction of its...Ch. 18.1 - Practice Problem CONCEPTUALIZE
Which equation is...Ch. 18.2 - Practice ProblemATTEMPT Calculate the standard...Ch. 18.2 - Practice Problem BUILD
In each of the following...Ch. 18.2 - Practice Problem CONCEPTUALIZE
For each reaction...Ch. 18.3 - Practice ProblemATTEMPT For each of the following...Ch. 18.3 - Practice Problem BUILD
Make a qualitative...Ch. 18.3 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 18.3 - 18.3.1 For which of the following physical...
Ch. 18.3 - 18.3.2 For which of the following chemical...Ch. 18.3 - 18.3.3 Identify the correct balanced equation and...Ch. 18.4 - Practice Problem ATTEMPT For each of the...Ch. 18.4 - Practice Problem BUILD (a) Calculate Δ S univ and...Ch. 18.4 - Practice Problem CONCEPTUALIZE The following table...Ch. 18.4 - Using data from Appendix 2, calculate Δ S ° (in...Ch. 18.4 - 18.4.2 Using data from Appendix 2, calculate (in...Ch. 18.4 - The diagrams show a spontaneous chemical reaction....Ch. 18.4 - 18.4.4 The diagrams show a spontaneous chemical...Ch. 18.5 - Practice Problem ATTEMPT
A reaction will be...Ch. 18.5 - Practice Problem BUILD
Given that the reaction is...Ch. 18.5 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 18.5 - A reaction for which Δ H and Δ S are both negative...Ch. 18.5 - At what temperature ( in ºC ) does a reaction go...Ch. 18.5 - 18.5.3 Using data from Appendix 2, calculate G°...Ch. 18.5 - 18.5.4 Calculate for the sublimation of iodine in...Ch. 18.6 - Practice Problem ATTEMPT
Calculate the standard...Ch. 18.6 - Practice problemBUILD For each reaction, determine...Ch. 18.6 - Prob. 1PPCCh. 18.6 - 18.6.1 For the reaction:
Ch. 18.6 - Consider the reaction: X ( g ) + Y(g) ⇄ Z( g ) for...Ch. 18.6 - The Δ G° for the reaction: N 2 ( g ) + 3H 2 (g) ⇄...Ch. 18.6 - 18.6.4 The for iron(III) hydroxide . For the...Ch. 18.7 - Practice Problem ATTEMPT
The molar heats of fusion...Ch. 18.7 - Practice Problem CONCEPTUALIZE
Explain why. in...Ch. 18.8 - Practice ProblemATTEMPT Δ G ° for the reaction: H...Ch. 18.8 - Practice ProblemBUILD What is the minimum partial...Ch. 18.8 - Practice Problem CONCEPTUALIZE Consider the...Ch. 18.9 - Practice Problem ATTEMPT Using data from Appendix...Ch. 18.9 - Practice ProblemBUILD K f for the complex ion Ag (...Ch. 18.9 - Practice Problem CONCEPTUALIZE Which of the...Ch. 18.10 - Practice ProblemATTEMPT Calculate G for the...Ch. 18.10 - Practice ProblemBUILD Ksp for Co(OH)2 at...Ch. 18.10 - Prob. 1PPCCh. 18 - 18.1
Which of the following must be negative for a...Ch. 18 - Δ G for a reaction is always negative when (a) Δ G...Ch. 18 - 18.3
The diagram shown here depicts a system at...Ch. 18 - The reaction shown here has Δ G º = -1 .83 kJ/mol...Ch. 18 - 18.1 Explain what is meant by a spontaneous...Ch. 18 - Prob. 2QPCh. 18 - Prob. 3QPCh. 18 - Describe what is meant by the term entropy. What...Ch. 18 - Prob. 5QPCh. 18 - Prob. 6QPCh. 18 - Prob. 7QPCh. 18 - Prob. 8QPCh. 18 - How does the entropy of a system change for each...Ch. 18 - Prob. 10QPCh. 18 - Prob. 11QPCh. 18 - Prob. 12QPCh. 18 - Prob. 13QPCh. 18 - Using the data in Appendix 2, calculate the...Ch. 18 - 18.15 Using the data in Appendix 2, calculate the...Ch. 18 - Prob. 16QPCh. 18 - Prob. 17QPCh. 18 - Prob. 18QPCh. 18 - 18.19 State the third law of thermodynamics in...Ch. 18 - Calculate Δ S surr for each of the reactions in...Ch. 18 - Calculate Δ S surr for each of the reactions in...Ch. 18 - Using data from Appendix 2, calculate Δ S rxn º...Ch. 18 - 18.23 Using data from Appendix 2, calculate for...Ch. 18 - Prob. 24QPCh. 18 - Why is it more convenient to predict the direction...Ch. 18 - What is the significance of the sign of Δ G sys ?Ch. 18 - From the following combinations of Δ H and Δ S ,...Ch. 18 - Prob. 28QPCh. 18 - Prob. 29QPCh. 18 - From the values of Δ H and Δ S , predict which of...Ch. 18 - Find the temperatures at which reactions with the...Ch. 18 - The molar heats of fusion and vaporization of...Ch. 18 - 18.33 The molar heats of fusion and vaporization...Ch. 18 - Prob. 34QPCh. 18 - Prob. 35QPCh. 18 - Prob. 36QPCh. 18 - Prob. 37QPCh. 18 - Prob. 38QPCh. 18 - Explain why Equation 18.14 is of great importance...Ch. 18 - Prob. 40QPCh. 18 - Prob. 41QPCh. 18 - Prob. 42QPCh. 18 - 18.43 Consider the following reaction at...Ch. 18 - Prob. 44QPCh. 18 - 18.45
(a)
Calculate and for the following...Ch. 18 - Prob. 46QPCh. 18 - Consider the decomposition of calcium carbonate:...Ch. 18 - Prob. 48QPCh. 18 - 18.49 At for the process:
is 8.6 kJ/mol....Ch. 18 - Prob. 50QPCh. 18 - What is a coupled reaction? What is its importance...Ch. 18 - What is the role of ATP in biological reactions?Ch. 18 - Prob. 53QPCh. 18 - 18.54 In the metabolism of glucose, the first step...Ch. 18 - Predict the signs of Δ H , Δ S , and Δ G of the...Ch. 18 - Prob. 56APCh. 18 - Prob. 57APCh. 18 - Prob. 58APCh. 18 - Prob. 59APCh. 18 - Prob. 60APCh. 18 - Ammonium nitrate ( NH 4 NO 3 ) dissolves...Ch. 18 - 18.62 Calculate the equilibrium pressure of due...Ch. 18 - Prob. 63APCh. 18 - Referring to Problem 18.63, explain why the ratio...Ch. 18 - 18.65 Which of the following are not state...Ch. 18 - 18.66 For reactions carried out under...Ch. 18 - Prob. 67APCh. 18 - Prob. 68APCh. 18 - A student looked up the Δ G f o , Δ H f o , and Δ...Ch. 18 - Consider the following Brønsted acid-base reaction...Ch. 18 - 18.71 At o K, the entropy of carbon monoxide...Ch. 18 - Prob. 72APCh. 18 - Consider the thermal decomposition of CaCO 3 :...Ch. 18 - Prob. 74QPCh. 18 - Prob. 75QPCh. 18 - Prob. 76QPCh. 18 - Prob. 77APCh. 18 - Prob. 78APCh. 18 - Prob. 79APCh. 18 - Prob. 80APCh. 18 - Prob. 81APCh. 18 - Prob. 82APCh. 18 - 18.83 Comment on the statement: “Just talking...Ch. 18 - Prob. 84APCh. 18 - Consider the reaction: N 2 ( g ) + O 2 ( g ) ⇄ 2...Ch. 18 - Prob. 86APCh. 18 - Consider the decomposition of magnesium carbonate:...Ch. 18 - Prob. 88APCh. 18 - Prob. 89APCh. 18 - 18.90 The rate constant for the elementary...Ch. 18 - A 74.6-g ice cube floats in the Arctic Sea. The...Ch. 18 - 18.92 Which of the following is not accompanied by...Ch. 18 - Prob. 93APCh. 18 - Give a detailed example of each of the following,...Ch. 18 - Prob. 95QPCh. 18 - 18.96 The standard enthalpy of formation and the...Ch. 18 - Prob. 97QPCh. 18 - Prob. 98QPCh. 18 - The following reaction was described as the cause...Ch. 18 - Comment on the feasibility of extracting copper...Ch. 18 - 18.101 One of the steps in the extraction of iron...Ch. 18 - Prob. 102APCh. 18 - Prob. 103APCh. 18 - Prob. 104APCh. 18 - 18.105 The enthalpy change in the denaturation of...Ch. 18 - Prob. 106APCh. 18 - Prob. 107APCh. 18 - Prob. 108APCh. 18 - Prob. 109APCh. 18 - Prob. 110APCh. 18 - 18.111 Carbon monoxide and nitric oxide are...Ch. 18 - Prob. 112APCh. 18 - Prob. 113APCh. 18 - 18.114 Many hydrocarbons exist as structural...Ch. 18 - Physical and Biological Sciences
In chemistry, the...Ch. 18 - Physical and Biological Sciences
In chemistry, the...Ch. 18 - Prob. 3SEPPCh. 18 - Physical and Biological Sciences
In chemistry, the...
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- I keep getting 2 different answers can u please verify for me which is right? -1.69 or different onearrow_forwardBe sure to answer all parts. 0 Calculate AG for each reaction using AG values: f (a) H₂(g) + I₂ (s) (b) MnO₂(s) + 2CO(g) ->> Mn(s) + 2CO₂(g) (c) NH4Cl(s) NH3(g) + HCI(g) Substance ->> Standard Thermodynamic Values at 298 K AG (kJ/mol) f CO(g) CO₂(g) CO,(aq) HCl(g) HCl(aq) HI(g) MnO₂ (s) NH3(g) NH3(aq) NH4Cl(s) 2HI(g) ㅍ El -137.2 -394.4 -386.2 -95.30 -131.17 1.3 -466.1 -16 26.7 -203.0 H kJ kJ kJ Prev 10arrow_forwardAre the following redox reactions spontaneous under standard conditions?(a) Zn(s) + Ni2+(aq)------>Zn2+(aq) + Ni(s)(b) Zn(s) + Ca2+(aq)--------->Zn2+(aq) + Ca(s)arrow_forward
- Please correct answer and don't used hand raitingarrow_forwardQuestion 4 4.1 When 0.50 mol of an ideal gas is expanded isothermally and reversibly at 298 K from a volume of 10.0 L to 25.0 L, (a) What is the 4Sgas? (b) How much work was done? (c) What is the 4Ssurr? (d) What is the 4Stotal? 4.2 At 25.0 °C the equilibrium constant for the reaction: CO(g) + H₂O(g) = CO2(g) + H2(g) is 1.00 x 10-5, and AS° is 41.8 J K-1 mol-¹. Calculate 4Gº and AH° at 25.0 °C.arrow_forwardPart A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remainingarrow_forward
- (1) Calculate AG for the following reactions at the stated temperatures: (a) ZnO(s) + C(s) Zn(s) + CO(g) at 298 K, when AH08 +238.6 kJ mol; AS = +213 J K mol. (b) ZnO(s) + C(s) Zn(g) + CO(g) at 1373 K, when An = +349.9 kJ mol; AS3 = +285 J K- mol. (c) Fe(s) + 0,(8) FeO(s) at 298 K, when AH298 = -265.4 kJ mol; ASOR = -71 J K mol.arrow_forwardConsider the Gibbs energies at 25 ∘25 ∘C. SubstanceSubstance Δ?∘f (kJ·mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq) 77.1 Cl−(aq) −131.2 AgCl(s) −109.8 Br−(aq) −104.0 AgBr(s) −96.9 (a) Calculate Δ?∘rxn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl. (c) Calculate Δ?∘rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr.arrow_forwardHello, can you break down the attached problem?arrow_forward
- Nonearrow_forwardCalculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.(a) O2(g) + 2F2(g) ⟶ 2OF2(g) ΔG° = −9.2 kJ(b) I2(s) + Br2(l) ⟶ 2IBr(g) ΔG° = 7.3 kJ(c) 2LiOH(s) + CO2(g) ⟶ Li2 CO3(s) + H2 O(g) ΔG° = −79 kJ(d) N2 O3(g) ⟶ NO(g) + NO2(g) ΔG° = −1.6 kJ(e) SnCl4(l) ⟶ SnCl4(l) ΔG° = 8.0 kJarrow_forwardConsider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25Carrow_forward
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