Math  /  Algebra

Question11) 0.7515 moles of nitrogen gas and 0.1135 moles of methane gas are placed in a 171.6 ml container at 20.8C20.8^{\circ} \mathrm{C}. What is the partial pressure (atm) of nitrogen gas? A) 1.14 B) 0.473 C) 16.0 D) 106 E) 226

Studdy Solution
Use the ideal gas law to calculate the partial pressure of nitrogen gas. The ideal gas law is given by:
PV=nRT PV = nRT
Where: - P P is the pressure, - V V is the volume, - n n is the number of moles, - R R is the ideal gas constant (0.0821L atm/mol K0.0821 \, \text{L atm/mol K}), - T T is the temperature in Kelvin.
Rearrange the formula to solve for P P :
P=nRTV P = \frac{nRT}{V}
Substitute the values for nitrogen gas:
P=0.7515moles×0.0821L atm/mol K×293.95K0.1716L P = \frac{0.7515 \, \text{moles} \times 0.0821 \, \text{L atm/mol K} \times 293.95 \, \text{K}}{0.1716 \, \text{L}}
Calculate the partial pressure:
P=0.7515×0.0821×293.950.1716 P = \frac{0.7515 \times 0.0821 \times 293.95}{0.1716}
P18.1080.1716 P \approx \frac{18.108}{0.1716}
P105.55atm P \approx 105.55 \, \text{atm}
The closest answer choice is:
106 \boxed{106}

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