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SOLUTION:

Step 1: List the given values.

[tex]\begin{aligned} & P = \text{741 torr = 0.975 atm} \\ & V = \text{5.40 L} \\ & T = 44^{\circ}\text{C} = \text{317.15 K} \\ & mass = \text{7.10 g} \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{0.975 atm})(\text{5.40 L})}{\left(0.082057 \: \dfrac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\right)(\text{317.15 K})} \\ & = \text{0.20231 mol} \end{aligned}[/tex]

Step 3: Calculate the molar mass of the gas.

[tex]\begin{aligned} MM & = \frac{mass}{n} \\ & = \frac{\text{7.10 g}}{\text{0.20231 mol}} \\ & = \boxed{\text{35.1 g/mol}} \end{aligned}[/tex]

Hence, the molar mass of the gas is 35.1 g/mol.

[tex]\\[/tex]

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