Question

a 6.00 l tank at 6.08 °c is filled with 7.16 g of dinitrogen monoxide gas and 11.1 g of chlorine pentafluoride gas. you can assume both gases behave as ideal gases under these conditions. calculate the total pressure in the tank. round your answer to the correct number of significant digits. your answer total pressure in tank: atm

Explanation:

Step1: Convert temperature to Kelvin

$$T = 6.08 + 273.15=279.23\ K$$

Step2: Calculate moles of dinitrogen monoxide ($N_2O$)

Molar mass of $N_2O$ is $M_{N_2O}=(2\times14.01)+16.00 = 44.02\ g/mol$.
$$n_{N_2O}=\frac{7.16\ g}{44.02\ g/mol}\approx0.1627\ mol$$

Step3: Calculate moles of chlorine pentafluoride ($ClF_5$)

Molar mass of $ClF_5$ is $M_{ClF_5}=35.45+(5\times19.00)=130.45\ g/mol$.
$$n_{ClF_5}=\frac{11.1\ g}{130.45\ g/mol}\approx0.0851\ mol$$

Step4: Calculate total moles ($n_{total}$)

$$n_{total}=n_{N_2O}+n_{ClF_5}=0.1627 + 0.0851=0.2478\ mol$$

Step5: Use ideal gas law ($PV = nRT$) to find pressure ($P$)

$R = 0.0821\ L\cdot atm/(mol\cdot K)$, $V = 6.00\ L$
$$P=\frac{n_{total}RT}{V}=\frac{0.2478\ mol\times0.0821\ L\cdot atm/(mol\cdot K)\times279.23\ K}{6.00\ L}$$
$$P=\frac{0.2478\times0.0821\times279.23}{6.00}\ atm$$
$$P=\frac{5.739}{6.00}\ atm\approx0.957\ atm$$

Answer:

$0.957\ atm$