Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.

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Identify the reactants: aluminum metal (Al) and cobalt(II) sulfate (CoSO_4).

Determine the possible products: aluminum sulfate (Al_2(SO_4)_3) and cobalt metal (Co).

Consult the activity series to compare the reactivity of aluminum and cobalt. Aluminum is more reactive than cobalt.

Since aluminum is more reactive, it will displace cobalt from cobalt(II) sulfate, leading to a reaction.

Write the balanced chemical equation: 2Al(s) + 3CoSO_4(aq) \(\rightarrow\) Al_2(SO_4)_3(aq) + 3Co(s).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Activity Series

The activity series is a list of metals ranked by their ability to displace other metals from solutions of their ions. Metals higher in the series can displace those lower in the series. This concept is crucial for predicting whether a reaction will occur when a metal is added to a solution containing another metal's ions.

Single Replacement Reaction

A single replacement reaction occurs when one element replaces another in a compound. In the context of the activity series, if a more reactive metal is introduced to a solution containing a less reactive metal's ions, a reaction will take place, resulting in the formation of a new compound and the release of the less reactive metal.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is essential for accurately representing the conservation of mass during a chemical reaction. In the case of the reaction between aluminum and cobalt(II) sulfate, balancing the equation will confirm the stoichiometry of the products formed.