There are 45,000 mg of nitrogen dioxide in a container at stp. what is the volume?

V = 22.86 L

Explanation:

Given data:

Mass of nitrogen dioxide = 45000 mg

Pressure = 1 atm

Temperature = 273 k

Volume = ?

Solution:

First of all we will convert the mass into moles.

Number of moles = mass/ molar mass

Number of moles = 45 g/ 46 g/mol

Number of moles = 1.02 mol

Now we will determine the volume at STP.

PV = nRT

V = nRT/P

V =  1.02 mol × 0.0821 atm. mol⁻¹. k⁻¹. L× 273 k / 1 atm

V = 22.86 atm. L /1 atm

V = 22.86 L

no

explanation:

go away, people want answers, not to hook up

1 a

2 d

3 a

4 c

explanation: