SOLUTION:
Step 1: List the given values
[tex]\begin{aligned} & P = \text{0.987 atm} \\ & V = \text{65.9 mL = 0.0659 L} \\ & T = \text{276 K} \end{aligned}[/tex]
Step 2: Calculate the number of moles of gas using ideal gas equation.
[tex]\begin{aligned} n & = \frac{PV}{\text{RT}} \\ & = \frac{(\text{0.987 atm})(\text{0.0659 L})}{\left(0.082057 \: \dfrac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\right)(\text{276 K})} \\ & = \boxed{2.87 \times 10^{-3} \: \text{mol}} \end{aligned}[/tex]
Hence, the chemist produced 2.87 × 10⁻³ mol of the gas.
[tex]\\[/tex]
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