Chemistry: Solve the following, show all work and units for your calculation: Let s say we have a mixture of hydrogen gas(H2), and oxygen gas (O2). The mixture contains 6.7 mol hydrogen gas and 3.3 mol oxygen gas. The mixture isin a 300 L container at 273 K and the total pressure of the gas mixture is 0.75 atm. What is the partialpressure for each gas?

Solve the following, show all work and units for

zoilacarrillosfe14

26.01.2022

The partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

Explanation:

We are given:

Moles of hydrogen gas = 6.7 moles

Moles of oxygen gas = 3.3 moles

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

Mole fraction of hydrogen gas, $\chi_{H_2}=\frac{6.7}{6.7+3.3}=0.67$

Mole fraction of oxygen gas, $\chi_{O_2}=\frac{3.3}{6.7+3.3}=0.33$

To calculate the total pressure of the container, we use the equation given by Raoult's law, which is:

$p_{A}=p_T\times \chi_{A}$

where,

p_A = partial pressure of substance

p_T = total pressure

$\chi_A$ = mole fraction of substance

For hydrogen gas:

We are given:

$\chi_{H_2}=0.67\\p_T=0.75atm$

Putting values in above equation, we get:

$p_{H_2}=0.75atm\times 0.67=0.503atm$

For oxygen gas:

We are given:

$\chi_{O_2}=0.33\\p_T=0.75atm$

Putting values in above equation, we get:

$p_{O_2}=0.75atm\times 0.33=0.248atm$

Hence, the partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

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