What would be the pressure of 1.0g of o2 contained in a 4.00l container at 293 k?

The pressure will be equal to 0.19 atm.

Explanation:

The Ideal Gas Equation states the relationship among the pressure, temperature, volume, and number of moles of a gas.

The equation is:

where P = pressure in atm

           V = volume in L

           n = numbers of moles of gas in mol

           R = universal gas constant = 0.08206

           T = temperature in K

Based on the problem,

mass of O2 = 1.0 g

V = 4.00 L

T = 293 K

mol of O2  = ?

P = ?

We need to calculate the moles of O2 before we can use the Ideal Gas Equation. To solve the number of moles, we use the equation:

The molar mass of O2 is 32 g/mol, therefore,

no. of moles of O2 = 0.03125 mol.

Now we substitute the values into the Ideal Gas equation:

Solving for P, we will get

In correct significant figures, P is equal to 0.19 atm.

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