Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. a. 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g)
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Ch.6 - Thermochemistry
Chapter 6, Problem 89
During photosynthesis, plants use energy from sunlight to form glucose (C6H12O6) and oxygen from carbon dioxide and water. Write a balanced equation for photosynthesis.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Photosynthesis
Photosynthesis is the biochemical process by which green plants, algae, and some bacteria convert light energy into chemical energy. This process primarily occurs in the chloroplasts of plant cells, where chlorophyll captures sunlight to drive the conversion of carbon dioxide and water into glucose and oxygen.
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Balanced Chemical Equation
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Balancing ensures that the reactants and products are accurately represented.
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Reactants and Products
In a chemical reaction, reactants are the starting substances that undergo change, while products are the substances formed as a result of the reaction. In photosynthesis, the reactants are carbon dioxide and water, and the products are glucose and oxygen. Understanding the roles of reactants and products is essential for writing and balancing chemical equations.
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Related Practice
Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. b. SO2(g) + 1/2 O2(g) → SO3(g)
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Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. d. N2O4(g) + 4 H2(g) → N2(g) + 4 H2O(g)
Textbook Question
Ethanol (C2H5OH) can be made from the fermentation of crops and has been used as a fuel additive to gasoline. Write a balanced equation for the combustion of ethanol and calculate ΔH°rxn.
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Textbook Question
Top fuel dragsters and funny cars burn nitromethane as fuel according to the balanced combustion equation: 2 CH3NO2(l) + 3/2O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g) ΔH°rxn = –1418 kJ The enthalpy of combustion for nitromethane is –709.2 kJ/mol. Calculate the standard enthalpy of formation (ΔH°f ) for nitromethane.
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Textbook Question
The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the balanced equation: 4 C3H5N3O9(l) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) ΔH°rxn = –5678 kJ Calculate the standard enthalpy of formation (ΔH°f ) for nitroglycerin.
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