Question

a chemist determined by measurements that 0.0550 moles of silver participated in a chemical reaction. calculate the mass of silver that participated in the chemical reaction. round your answer to 3 significant digits.

Explanation:

Step1: Recall the formula for mass from moles

The formula to calculate mass from moles is \( \text{Mass} = \text{Moles} \times \text{Molar Mass} \). The molar mass of silver (Ag) is approximately \( 107.87 \, \text{g/mol} \).

Step2: Substitute the values into the formula

We have moles \( = 0.0550 \, \text{mol} \) and molar mass \( = 107.87 \, \text{g/mol} \). So, \( \text{Mass} = 0.0550 \, \text{mol} \times 107.87 \, \text{g/mol} \).

Step3: Perform the calculation

\( 0.0550 \times 107.87 = 6.03285 \, \text{g} \).

Step4: Round to 3 significant digits

Rounding \( 6.03285 \) to 3 significant digits gives \( 6.03 \, \text{g} \).

Answer:

\( 6.03 \, \text{g} \)