Multiple Choice
What is the correct coefficient for O_2(g) when balancing the following chemical equation: 2C_4H_{10}(g) + O_2(g) → 8CO_2(g) + 10H_2O(g)?
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3. Chemical Reactions
Balancing Chemical Equations
Multiple Choice
Which of the following best describes the reaction: 2 H_2S(g) + 3 O_2(g) → 2 H_2O(g) + 2 SO_2(g)?
A
It is a redox reaction in which hydrogen sulfide is oxidized and oxygen is reduced.
B
It is a double displacement reaction between hydrogen sulfide and oxygen.
C
It is a synthesis reaction forming water and sulfur dioxide from their elements.
D
It is a decomposition reaction where hydrogen sulfide breaks down into water and sulfur dioxide.
Verified step by step guidance1
Identify the reactants and products in the given chemical equation: \(2\ H_2S(g) + 3\ O_2(g) \rightarrow 2\ H_2O(g) + 2\ SO_2(g)\).
Determine the oxidation states of the elements in the reactants and products to see if there is a change, which indicates a redox reaction. For example, sulfur in \(H_2S\) and in \(SO_2\), and oxygen in \(O_2\) and in \(H_2O\) and \(SO_2\).
Check if electrons are transferred by identifying which species is oxidized (loses electrons) and which is reduced (gains electrons). Oxidation involves an increase in oxidation state, and reduction involves a decrease.
Analyze the type of reaction based on the changes: if electrons are transferred, it is a redox reaction; if ions exchange partners, it is a double displacement; if elements combine, it is synthesis; if a compound breaks down, it is decomposition.
Conclude that since hydrogen sulfide loses electrons (oxidized) and oxygen gains electrons (reduced), the reaction is a redox reaction where hydrogen sulfide is oxidized and oxygen is reduced.
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