Consider the reaction: C3H8(g) + 3 O₂(g) → CH4(g) + 2 CO₂(g) + 2H₂0(1), AH=-1330. kJ/mol. Using this information, compute the following: a. Heat of reaction at constant pressure (in kJ) when 3.000 moles of propane react with excess O₂ at 25 °C b. Heat of reaction at constant pressure (in kJ) when 25 moles of propane reacts with 1.5 moles of oxygen gas. C. The enthalpy of reaction, 4H, for: 2 CH4(g) + 4 CO₂(g) + 4H₂O(1) →2 C3H2(g) + 60₂(g) ½ C3H2(g) + 3/2 02(g) → ½ CH4(g) + CO₂(g) + H₂O(l) d. The enthalpy of reaction, 4H, for:
Consider the reaction: C3H8(g) + 3 O₂(g) → CH4(g) + 2 CO₂(g) + 2H₂0(1), AH=-1330. kJ/mol. Using this information, compute the following: a. Heat of reaction at constant pressure (in kJ) when 3.000 moles of propane react with excess O₂ at 25 °C b. Heat of reaction at constant pressure (in kJ) when 25 moles of propane reacts with 1.5 moles of oxygen gas. C. The enthalpy of reaction, 4H, for: 2 CH4(g) + 4 CO₂(g) + 4H₂O(1) →2 C3H2(g) + 60₂(g) ½ C3H2(g) + 3/2 02(g) → ½ CH4(g) + CO₂(g) + H₂O(l) d. The enthalpy of reaction, 4H, for:
Chemistry for Engineering Students
4th Edition
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Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.53PAE: 9.53 Using these reactions, find the standard enthalpy change for the formation of 1 mol of PhO(s)...
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Transcribed Image Text:Consider the reaction: C3H8(g) + 3 O₂(g) → CH4(g) + 2 CO₂(g) + 2H₂0(1), AH=-1330. kJ/mol. Using this
information, compute the following:
a.
Heat of reaction at constant pressure (in kJ) when 3.000 moles of propane react with excess O₂ at 25 °C
b. Heat of reaction at constant pressure (in kJ) when 25 moles of propane reacts with 1.5 moles of oxygen gas.
C. The enthalpy of reaction, 4H, for: 2 CH4(g) + 4 CO₂(g) + 4H₂O(1) →2 C3H³(g) + 60₂(g)
d. The enthalpy of reaction, 4H, for: ½ C3H2(g) + 3/2 02(g) →→→ ½ CH4(g) + CO₂(g) + H₂O(l)
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