A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container?

The ideal gas law, also called the general gas equation, is the equation of the state of a hypothetical ideal gas.

The ideal gas law work under the constant:-  

Hence the formula we gonna use is as follows:-

In the question, the pressure, temperature, and volume are given in two different systems.

As the date given in the question, after putting it into the equation:-

n= 0.271.

The number of moles in the nitrogen container is 0.271.

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n = 0.271 moles

Explanation:

Given that,

Volume of container, V = 14 L

Pressure of Nitrogen gas, P = 375 torr

Temperature. T = 37°C=37+273=310°C

We need to find the number of moles of nitrogen in the container. Using gas equation,

PV = nRT

R is gas constant, R = 0.082 L-atm/mol-K

Since, 1 atm=760 torr

375 torr = 0.493 atm

Now,

So, there are 0.271 moles of Nitrogen in the container.

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: