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3 months ago

What is the mass of 22.4 L of H2 at STP?

Chemistry

2 answers:

eduard [2.7K]3 months ago

7 0

A. 1.01 is the accurate result

Because

The formula used is Pv= nRT

P=1 atm

V= 22.4 L

N= x

R= 0.0821

T= 273 K (since it’s standard temperature)

Thus, (1)(22.4)=(x)(0.0821)(273)

X= 1.001

KiRa [2.9K]3 months ago

6 0

Answer: The correct choice is option (b).

Explanation:

STP refers to standard temperature and pressure. Under these conditions, pressure is set at 1 atm, volume at 22.4 L, and temperature at 298 K.

Consequently, by using the ideal gas equation, we can compute the number of moles as follows.

PV = nRT

$1 atm \times 22.4 L = n \times 0.0832 Latm K^{-1}mol^{-1} \times 298K$

n = 0.903 mol

≈ 1 mol

Therefore, given that the molar mass of a hydrogen molecule is 2 g/mol, we can calculate the mass of $H_{2}$ at STP as follows.

Number of moles = $\frac{mass}{molar mass}$

1 mol = $\frac{mass}{2.02 g/mol}$

mass = 2.02 g

Thus, we can conclude that the mass of 22.4 L of H2 at STP is 2.02 grams.

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