A 0.316 mol sample of nitrogen gas, N2 (g), is placed in a 4.00 L container at 315 K.

2.04 atm is the pressure of the nitrogen gas in the container when 0.316 mol sample of nitrogen gas, N2 (g), is placed in a 4.00 L container at 315 K.

Explanation:

Data given:

moles of nitrogen gas, n = 0.316

volume of the nitrogen gas, V = 4 litres

temperature of the container of nitrogen gas  = 315 K

R (gas constant) = 0.08201 Latm/mole K

Pressure of the nitrogen gas on the container,  P = ?

from the data given, we will apply ideal gas law equation to calculate the pressure on the nitrogen gas:

PV = nRT

Rearranging the equation,

P =

P =

P = 2.04 atm

The pressure of the nitrogen gas in the container is 2.04 atm.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

yes

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