(a) Interpretation Introduction To determine: The energy stored by photosynthesis on land in one year. Explanation Given The amount of carbon dioxide produced by the plant is 5.5 × 10 16 g/yr . The molar mass of carbon dioxide is, 12.0 g/mol + 2 × 16.0 g/mol = 44.0 g/mol The balanced chemical equation for the conversion of carbon dioxide into glucose is, 6 CO 2 ( g ) + 6 H 2 O ( l ) → C 6 H 12 O 6 ( s ) + 6 O 2 ( g ) The enthalpy change of the given reaction is calculated by the formula, Δ H ∘ = ∑ n Δ H ∘ ( products ) − ∑ m Δ H ∘ ( reactants ) = ( Δ H C 6 H 12 O 6 ( s ) ∘ + 6 Δ H O 2 ( g ) ∘ ) − ( 6 Δ H CO 2 ( g ) ∘ + 6 Δ (b) Interpretation Introduction To determine: The rate of conversion of solar energy into plant energy; also the number of nuclear plants in the solar energy conversion.

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ISBN: 9781323233252

Author: Brown

Publisher: PEARSON C

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Chapter 14, Problem 54E

(a)

Interpretation Introduction

To determine: The energy stored by photosynthesis on land in one year.

(b)

Interpretation Introduction

To determine: The rate of conversion of solar energy into plant energy; also the number of nuclear plants in the solar energy conversion.

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Chapter 14, Problem 53E

Chapter 14, Problem 55E

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The two equations are forms of the Davies equation, used in thermodynamics for activity coefficients: ال log Y₁ = -Az² - 0,31 log = Az² - 0,31 1 + √Ĩ 1 + √√ k These equations are consistent and imply that Yi = Is this last equation correct? k

For the Davies equation, both expressions are correct: log Y₁ = -Az² √i - 0,31 1 + √ k log- = Az - 0,31 k 1 + √Ĩ

k In Davies' equation log y₁ = log- log y₁ = log | = -Az² + ✓// k A is a constant that always equals 1.02. Correct? - 0,31

Chapter 14 Solutions

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Ch. 14.2 - Identify the force present and explain whether...Ch. 14.2 - Identify the force present and explain whether...Ch. 14.2 - Which of the following cannot leave or enter a...Ch. 14.2 - Prob. 14.2.2PE Ch. 14.2 - According to the first law of thermodynamics, what...Ch. 14.2 - Write an equation that expresses the first law of...Ch. 14.3 - Calculate AB and determine whether the process is...Ch. 14.3 - For the following processes, calculate the change...Ch. 14.3 - A gas is confined to a cylinder fitted with a...Ch. 14.3 - Consider a system consisting of two oppositely...

Ch. 14.3 - Prob. 14.6.1PE Ch. 14.3 - Indicate which of the following is independent of...Ch. 14.4 - During a normal breath, our lungs expand about...Ch. 14.4 - How much work (in J) is involved in a chemical...Ch. 14.4 - Why is the change in enthalpy usually easier to...Ch. 14.4 - Under what condition will the enthalpy change of a...Ch. 14.4 - Assume that the following reaction occurs at...Ch. 14.4 - Suppose that the gas-phase reaction 2NO(g) + 02(g)...Ch. 14.5 - Which of the following statements is or are true?...Ch. 14.5 - Prob. 14.10.2PE Ch. 14.5 - In the accompanying cylinder diagram, a chemical...Ch. 14.5 - Prob. 14.11.2PE Ch. 14.6 - Consider the two diagrams that follow. Based on...Ch. 14.6 - Consider the conversion of compound A into...Ch. 14.6 - What is the electrostatic potential energy (in...Ch. 14.6 - What is the electrostatic potential energy (in...Ch. 14.6 - Prob. 14.14.1PE Ch. 14.6 - Use the equations given in Problem 5.15 to...Ch. 14.6 - A sodium ion, Na+, with a charge of 1.6 x 10-19 C...Ch. 14.6 - A magnesium ion, Mg2+, with a charge of 3.2 x...Ch. 14 - 5.74 Using values from Appendix C, calculate the...Ch. 14 - Complete combustion of 1 mol of acetone (C2H6O)...Ch. 14 - 5.87 Consider the reaction 2H(g) + O2(g) ...Ch. 14 - The air bags that provide protection in...Ch. 14 - 5.111 From the following data for three...Ch. 14 - 5.123 Consider two solutions, the first being...Ch. 14 - For each of the following transitions, give the...Ch. 14 - In this chapter, we have learned about the...Ch. 14 - 6.12 State where in the periodic table these...Ch. 14 - Einstein's 1905 paper on the photoelectric effect...Ch. 14 - 5.48 Consider the decomposition of liquid...Ch. 14 - Under constant-volume conditions, the heat of...Ch. 14 - Given the data use Hess's law to calculate H for...Ch. 14 - 5.67 What is meant by the term standard...Ch. 14 - S 5.68 What is the value of the standard enthalpy...Ch. 14 - For each of the following compounds, write a...Ch. 14 - Write balanced equations that describe the...Ch. 14 - The following is known as the thermite reaction:...Ch. 14 - (a) What are the units usually used to express the...Ch. 14 - Using values from Appendix C , calculate the...Ch. 14 - 5.77 Gasoline is composed primarily of...Ch. 14 - Prob. 21E Ch. 14 - Ethanol (C2H5OH) is blended with gasoline as an...Ch. 14 - 5.80 Methanol (CH3OH) is used as a fuel in race...Ch. 14 - 5.81 Without doing any calculations, predict the...Ch. 14 - 5.82 Without doing any calculations, predict...Ch. 14 - Use bond enthalpies in Table 5.4 Q to estimate for...Ch. 14 - Use bond enthalpies in Table 5.40 to estimate for...Ch. 14 - Use enthalpies of formation given in Appendix C to...Ch. 14 - 5.86 The nitrogen atoms in an N2 molecule are...Ch. 14 - 5.89 What is meant by the term fuel value? 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What is...Ch. 14 - 5.52 a. Which substance in Table 5.2 requires...Ch. 14 - The specific heat of octane, C8H18(l), is 2.22...Ch. 14 - 6.54 Consider the data about gold metal in...Ch. 14 - When a 6-50-g sample of solid sodium hydroxide...Ch. 14 - 5.56 a. When a 4 25-g sample of solid ammonium...Ch. 14 - A 2.200-g sample of quinone (C5H402) is burned in...Ch. 14 - 8.68 A 1.800-g sample of phenol (C6H5OH) was...Ch. 14 - 5.60 Under constant-volume conditions, the heat...Ch. 14 - 5.61 Can you use an approach similar to Hess's...Ch. 14 - 5.62 Consider the following hypothetical...Ch. 14 - Calculate the enthalpy change for the reaction...Ch. 14 - From the enthalpies of reaction calculate H for...Ch. 14 - From the enthalpies of reaction Calculate H for...

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