The correct answer to this question is communicating
The answer to that question is v*140.187 moles of hydrogen.
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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.
It reacts well with the leftover hydrogen chloride in the stomach. It's also non-toxic. The products formed by the reaction are also non-toxic.