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11 Dec 2019

The combustion of hexane (C₆H₁₄), a component of gasoline, is represented by the balanced chemical equation:

If one mole of hexane undergoes combustion, how many moles of O₂ are required?

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Consider the following unbalanced equation for the combustion of hexane: C6H14(g)+O2(g)âCO2(g)+H2O 1- balance the equation 2- Determine how many moles of O2 are required to react completely with 5.2 moles C6H14

A scientist burns 0.315 moles of hexane (C6H14) inside a small chamber surrounded by 5.65 litres of water. What is the molar heat of combustion of hexane if the water temperature rises by 55.4oC?

Consider the unbalanced equation for the combustion of hexane:

αC6H14(g)+βO2(g)→γCO2(g)+δH2O(g)

Part A: Balance the equation using the least possible integers for coefficients.

Part B: Determine how many moles of O2 are required to react completely with 6.4 moles C6H14. Express your answer using two significant figures.

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The combustion of hexane (C₆H₁₄), a component of gasoline, is represented by the balanced chemical equation:

If one mole of hexane undergoes combustion, how many moles of O₂ are required?

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The combustion of hexane (C6H14), a component of gasoline, is represented by the balanced chemical equation: If one mole of hexane undergoes combustion, how many moles of O2 are required?

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

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The combustion of hexane (C₆H₁₄), a component of gasoline, is represented by the balanced chemical equation:

If one mole of hexane undergoes combustion, how many moles of O₂ are required?