Organic Chemistry
5th Edition
ISBN: 9780078021558
Author: Janice Gorzynski Smith Dr.
Publisher: McGraw-Hill Education
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Chapter 6, Problem 6.8P
Interpretation Introduction
(a)
Interpretation: The
Concept introduction: The
Interpretation Introduction
(b)
Interpretation: The
Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by
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To a test tube containing 5.0 ml of 1.00 M NaOH at 27°C in a calorimeter, 5.0 ml of 2.00 M HNO3 at the same temperature was added, the heat generated by the reaction was monitored. Which of the following is TRUE?
a.Reaction is exothermic; solution will turn pink upon addition of phenolphthalein.
b.Heat is absorbed by the system; no color change will be observed upon addition of phenolphthalein.
c.Heat is released by the system; no color change will be observed upon addition of phenolphthalein.
d.Reaction is endothermic; solution will turn pink upon addition of phenolphthalein.
Fe2O3(s) + 3CO(s) → 2Fe(s) + 3CO2(g) ΔH = -28.0 kJ
3Fe(s) + 4CO2(s) → Fe3O4(s) + 4CO(g) ΔH = +12.5 kJ
The enthalpy of reaction of Fe2O3 with CO
3Fe2O3(s) + CO(g) → CO2(g) + 2Fe3O4(s)
is ____kJ.
Consider the following reaction:2CH3OH(g)→2 CH4(g) + O2(g) H=+252.8 kJ
a. Is this reaction exothermic or endothermic? Explain briefly.
b. Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure
c. For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane, CH4, are produced?
d. How many kilojoules of heat are released when 38.5 g of CH4 (g) reacts completely with O2 (g) to form CH3OH( g) at constant pressure?
Chapter 6 Solutions
Organic Chemistry
Ch. 6 - Problem 6.1 Classify each transformation as...Ch. 6 - Prob. 6.2PCh. 6 - Problem 6.3 By taking into account...Ch. 6 - Problem 6.4 Use curved arrows to show the movement...Ch. 6 - Problem 6.5 Follow the curved arrows and draw the...Ch. 6 - Prob. 6.6PCh. 6 - Problem 6.7 Use the values in Table 6.2 to...Ch. 6 - Prob. 6.8PCh. 6 - aWhich Keq corresponds to a negative value of G,...Ch. 6 - Given each of the following values, is the...
Ch. 6 - Given each of the following values, is the...Ch. 6 - The equilibrium constant for the conversion of the...Ch. 6 - Prob. 6.13PCh. 6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6 - Draw an energy diagram for a reaction in which the...Ch. 6 - Prob. 6.17PCh. 6 - Prob. 6.18PCh. 6 - Problem 6.19 Consider the following energy...Ch. 6 - Draw an energy diagram for a two-step reaction,...Ch. 6 - Which value if any corresponds to a faster...Ch. 6 - Prob. 6.22PCh. 6 - Problem 6.23 For each rate equation, what effect...Ch. 6 - Prob. 6.24PCh. 6 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 6.29PCh. 6 - 6.30 Draw the products of each reaction by...Ch. 6 - 6.31 (a) Add curved arrows for each step to show...Ch. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Calculate H for each reaction. a HO+CH4CH3+H2O b...Ch. 6 - Homolysis of the indicated CH bond in propene...Ch. 6 - Prob. 6.37PCh. 6 - Prob. 6.38PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 6.40PCh. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 6.45PCh. 6 - Draw an energy diagram for the Bronsted-Lowry...Ch. 6 - Prob. 6.47PCh. 6 - Indicate which factors affect the rate of a...Ch. 6 - Prob. 6.49PCh. 6 - 6.50 The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 6.51PCh. 6 - Prob. 6.52PCh. 6 - The conversion of (CH3)3Cl to (CH3)2C=CH2 can...Ch. 6 - 6.54 Explain why is more acidic than , even...Ch. 6 - Prob. 6.55PCh. 6 - Prob. 6.56PCh. 6 - Prob. 6.57PCh. 6 - Although Keq of equation 1 in problem 6.57 does...Ch. 6 - Prob. 6.59P
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- The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy, ΔH, changes sign when a process is reversed. Consider the reaction H2O(l)→H2O(g), ΔH =44.0kJ What will ΔH be for the reaction if it is reversed?arrow_forwardCH,(9) + 2 O,(g) AH = -809.0 kJ/mol rxn Co,(9) + 2 H,0(g) ΔΗ. = -81.3 kJ 'cond 2 H,0U) Given the energy diagram above, what is AH when two moles of methane are combusted? -401.15 kJ +1604.6 kJ -802.3 kJ +802.3 kJ +401.15 kJ O -1604.6 kJarrow_forwardGiven the listed average bond energies (BE), calculate the enthalpy change for the production of one mole of methanol (CH3OH) by the following reaction. (There are two C=O double bonds in CO2) CO2(g) + 3 H2(g) → CH3OH(g) + H2O(g) B.E.C–O = 300 kJ/mol B.E.C=O = 700 kJ/mol B.E.H–H = 450 kJ/mol B.E.H–O = 500 kJ/mol B.E.H–C = 400 kJ/mol Select one: a. -250 kJ b. -950 kJ c. 950 kJ d. 50 kJ e. 250 kJarrow_forward
- Write a balanced equation for the formation of CO2(g) from C(s) and O2(g). Calculate the enthalpy change for this reaction using the following data (at 25 degrees Celsius): C(s) + 1/2 O2(g) --> CO(g) change in H = -111 kJ CO(g) + 1/2 O2(g) --> CO2(g) change in H = -394 kJ Is the reaction endothermic or exothermic?arrow_forwardUse the following information to answer question 5. Kerosene, C₁2H26(1), is a hydrocarbon used in jet fuel. The combustion of kerosene can be represented by the following equation. 2 C12H26(1) + 370₂(g) → 24 CO₂(g) + 26 H₂O(g) + 15 029.0 kJ 5. The enthalpy change for the combustion of 1.00 kg of kerosene is A. B. C. D. Not typed, just handwritte pls. -8.82 × 10¹ kJ -4.41 x 10¹ kJ +4.41 x 10¹ kJ +8.82 x 10 kJ -arrow_forward85. Propane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 °C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: We will see how to do this calculation in a later chapter on gases—for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of O2 per liter.) (c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation, ΔH∘fΔHf° of propane given that ΔH∘fΔHf° of H2O(l) = −285.8 kJ/mol and ΔH∘fΔHf° of CO2(g) = −393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.arrow_forward
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