Question

a chemist determined by measurements that 0.0700 moles of aluminum participated in a chemical reaction. calculate the mass of aluminum that participated in the chemical reaction.
be sure your answer has the correct number of significant digits.

Explanation:

Step1: Recall the formula for mass calculation

The formula is \( m = n\times M \), where \( m \) is mass, \( n \) is the number of moles, and \( M \) is the molar mass. The molar mass of aluminum (\(Al\)) is \( M = 26.98\space g/mol\).

Step2: Substitute the values into the formula

Given \( n=0.0700\space mol\) and \( M = 26.98\space g/mol\), we have \( m=0.0700\times26.98\).

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Step3: Round to the correct number of significant digits

The number \(0.0700\) has three significant digits. So, \(m = 1.89\space g\) (rounded to three significant digits).

Answer:

\(1.89\space g\)