### Thermochemistry of Butane Combustion**Problem Statement:**Butane, the fuel used in cigarette lighters, combusts according to the following thermochemical equation:\[ 2 \, \text{C}_4\text{H}_{10(g)} + 13 \, \text{O}_{2(g)} \rightarrow 8 \, \text{CO}_{2(g)} + 10 \, \text{H}_2\text{O}_{(g)} \quad \Delta H^\circ = -5316.6 \, \text{kJ} \]If 10.0 g of butane burns completely in oxygen and the heat is used to warm up 25.0 L of water at 22.0 °C, what will be the final temperature of the water (assuming that no heat is lost to the surroundings and that \(d = 1.00 \, \text{g/mL} \) for water)?**Analysis and Calculations:**1. **Understanding the Reaction:** - The combustion of butane is an exothermic reaction, releasing a significant amount of energy (\(-5316.6 \, \text{kJ}\)).2. **Heat Transfer to Water:** - 10.0 g of butane is used, and this energy will heat 25.0 L of water. - Convert 25.0 L of water to grams: \( 25,000 \, \text{g} \) (assuming \(d = 1.00 \, \text{g/mL} \)).3. **Calculate Moles of Butane:** - Molar mass of butane (C\(_4\)H\(_{10}\)): approximately \(58.12 \, \text{g/mol}\). - Moles of butane in 10.0 g: \[ \frac{10.0 \, \text{g}}{58.12 \, \text{g/mol}} \approx 0.172 \, \text{mol} \]4. **Energy Released:** - Total energy released by 0.172 mol of butane: \[ (0.172 \, \text{mol}) \times \left(\frac{-5316.6 \, \text{kJ}}{2 \

Here 10 g of butane was combusted and heat produced is used for heating 25L water at 22°C. We have…

8. Butane, which is the fuel used in cigarette lighters, combusts according to the following thermochemical equation: 2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H₂O(g) AH = -5316.6 kJ LR If 10.0 g of butane burns completely in oxygen and the heat is used to warm up 25.0 L of water at 22.0 °C, what will be the final temperature of the water (assuming that no heat is lost to the surroundings and that d = 1.00 g/mL for water))?

8. Butane, which is the fuel used in cigarette lighters, combusts according to the following thermochemical equation: 2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H₂O(g) AH = -5316.6 kJ LR If 10.0 g of butane burns completely in oxygen and the heat is used to warm up 25.0 L of water at 22.0 °C, what will be the final temperature of the water (assuming that no heat is lost to the surroundings and that d = 1.00 g/mL for water))?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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