3. Given the thermochemical equation:SO₂(g) + O₂(g) → SO3(g)Calculate how much heat will be liberated when:a. ½ mole of SO₂ reactsb. 2 moles of SO₂ reacts4. Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines.From the following data, calculate the standard enthalpy of formation of methanol:2CH₂OH() + 30₂(g)2CO₂(g) + 4H₂O(l)AHxnAHxn=-99 kJAH-1452.8 kJA 7.3-g copper coin is at a temperature of 18.8°C. This coin is placed in 10.0 g of water at atemperature of 54.0°C. What is the final temperature of the coin and water, assuming no heat islost to the surroundings? Specific heat of water is 4.184 J/g*°C and specific heat of copper is0.385 J/g *°C.

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3. Given the thermochemical equation: SO₂(g) + O₂(g) → SO3(g) AHxn =-99 kJ Calculate how much heat will be liberated when: a. ½ mole of SO₂ reacts b. 2 moles of SO₂ reacts

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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Question

3. Given the thermochemical equation:
SO₂(g) + O₂(g) → SO3(g)
Calculate how much heat will be liberated when:
a. ½ mole of SO₂ reacts
b. 2 moles of SO₂ reacts
4. Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines.
From the following data, calculate the standard enthalpy of formation of methanol:
2CH₂OH() + 30₂(g)2CO₂(g) + 4H₂O(l)
AHxn
AHxn=-99 kJ
AH-1452.8 kJ
A 7.3-g copper coin is at a temperature of 18.8°C. This coin is placed in 10.0 g of water at a
temperature of 54.0°C. What is the final temperature of the coin and water, assuming no heat is
lost to the surroundings? Specific heat of water is 4.184 J/g*°C and specific heat of copper is
0.385 J/g *°C.

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