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Ch.3 - Chemical Reactions and Reaction Stoichiometry
All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 71
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Chapter 3, Problem 71

The complete combustion of octane, C8H18, produces 5470 kJ of heat. Calculate how many grams of octane are required to produce 20,000 kJ of heat.

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Step 1: Write the balanced chemical equation for the complete combustion of octane: \[ 2 \text{C}_8\text{H}_{18} + 25 \text{O}_2 \rightarrow 16 \text{CO}_2 + 18 \text{H}_2\text{O} \].
Step 2: Note that the combustion of 2 moles of octane produces 5470 kJ of heat. Therefore, calculate the heat produced per mole of octane by dividing 5470 kJ by 2.
Step 3: Determine the number of moles of octane needed to produce 20,000 kJ of heat by dividing 20,000 kJ by the heat produced per mole of octane calculated in Step 2.
Step 4: Calculate the molar mass of octane (C8H18) by adding the atomic masses of carbon (C) and hydrogen (H): \[ 8 \times 12.01 \text{ g/mol} + 18 \times 1.01 \text{ g/mol} \].
Step 5: Convert the moles of octane needed (from Step 3) to grams by multiplying the number of moles by the molar mass of octane calculated in Step 4.
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Textbook Question

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O2 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)?

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Textbook Question

The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g). (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted? (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted?

Textbook Question

Detonation of nitroglycerin proceeds as follows: 4 C3H5N3O91l2¡ 12 CO21g2 + 6 N21g2 + O21g2 + 10 H2O1g2 (a) If a sample containing 2.00 mL of nitroglycerin 1density = 1.592 g>mL2 is detonated, how many moles of gas are produced?

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Textbook Question

The combustion of one mole of liquid octane, CH3(CH2)6CH3, produces 5470 kJ of heat. Calculate how much heat is produced if 1.000 gallon of octane is combusted.

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Textbook Question

(a) Define the terms limiting reactant and excess reactant.

Textbook Question

(b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant?

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