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.

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.