Question

one dm3 of O2 at STP has mass? ​

Answer 1

Answer:

You will need the molar volume of a gas at STP in order to convert volume to moles. Then multiply by the molar mass of O2 gas to calculate its mass.

At STP defined as 273.15 K (0°C) and 1 atm, the molar volume of a gas is 22.4 dm^3/mol (22.4 L/mol).

Molar mass O2 = (2 × 15.999 g/mol O) = 31.998 g/mol O

Use dimensional analysis to convert volume of O2 gas to mass O2 gas.

134.5 dm^3 O2 × 1 mol O2/22.4 dm^3 O2 × 31.998 g O2/1 mol O2 = 192 g O2 to three significant figures

At STP of 273.15 K and 1 atm, 134.5 dm^3 O2 gas has a mass of ~192 g.

Explanation:

Answer 2

Answer:

14.3 g

Explanation:

STP represents Standard temperature and pressure conditions that are used to compare the results of experimentation at different places or with different set of data.

STP conditions are usually taken 273.15 K temperature and 1 atm pressure. At these conditions, volume of 1 mole of an ideal gas is found to be 22.4 L.

It means 22.4 L gas = 1 mole gas.

Now, convert 22.4 L into $dm^{3}$.

1 L = 1  $dm^{3}$

That means 22.4 L = 22.4  $dm^{3}$.

Next , it can be said that 22.4  $dm^{3}$ $O_{2}$ = 1 mole $O_{2}$ = 32.0 g $O_{2}$

Therefore, 1  $dm^{3}$ will contain-

$Mass\ of\ O_{2} =\frac{32.0\ g}{22.4\ dm^{3} }$×$1 dm^{3}$ =$1.43\ g$

Hence, one  $dm^{3}$ of $O_{2}$ has 1.43 g mass.

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