Makahanap ng mga eksaktong solusyon sa iyong mga problema gamit ang IDNStudy.com. Makakuha ng impormasyon mula sa aming mga eksperto, na nagbibigay ng maaasahang sagot sa lahat ng iyong mga tanong.
Step 1: List the given values.
[tex]\begin{aligned} & P = \text{660. mmHg = 0.86842 atm} \\ & V = \text{1.00 L} \\ & T = 112.0^{\circ}\text{C} = \text{385.15 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{0.86842 atm})(\text{1.00 L})}{\left(0.082057 \: \dfrac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\right)(\text{385.15 K})} \\ & = \text{0.0275 mol} \end{aligned}[/tex]
Step 3: Calculate the mass of the gas.
The molar mass of N₂ is 28.0 g/mol.
[tex]\begin{aligned} \text{mass} & = n \times \text{MM} \\ & = \text{0.0275 mol} \times \text{28.0 g/mol} \\ & = \boxed{\text{0.770 g}} \end{aligned}[/tex]
Hence, 0.770 g of nitrogen would be required.
[tex]\\[/tex]
#CarryOnLearning