Question

A cylinder is filled with butane $100mL$ at $2.5atm$, $263K$ . During use 1 mole of gas per hour withdrawn. What is the final Pressure inside the cylinder after usage for 2 hours.

Answer 1

Hint: In this question we will be seeing about the Ideal Gas Laws and their law applications. We will see how to find the final pressure of the gas inside a cylinder after usage through the ideal gas laws and pressure-mole equation.

Complete step by step solution: Ideal Gas Equation is the equation characterizing the conditions of the hypothetical gases communicated numerically by the blends of experimental and physical constants. It is additionally called the overall gas condition. It tends to be defined as: "The ideal gas law is the equation of state of a hypothetical ideal gas. It is a decent estimate of the approximation of numerous gases under numerous conditions, despite the fact that it has a few restrictions".
First let us write down what is given to us.
We were given:
Weight of butane inside the cylinder, that is, $100mL$and, $1mol$ gas per hour was removed.
Hence, the Moles of Butane gas present after two hours of usage in the cylinder is $98mL$
We already know that,
 $\dfrac{P_1}{n_1} = \dfrac{P_2}{n_2}$
Let us substitute the values we have in the above equation:
 $\dfrac{2.5}{100} = \dfrac{P_2}{98}$
Let us bring the value that we need to find out to the left hand side of the equation and then shift all the known values to the right hand side of the equation:
${P_2} = 2.5\times \dfrac{98}{100}$
After simplification we get the value of ${P_2}$ as $2.45atm$
$ \Rightarrow {P_2} = 2.45atm$
Is the final pressure after usage of 2 hours.

Note: Ideal gases are only present on paper we cannot consider the ideal gas situation for the gases which are present in nature s many of the properties of ideal gas does not apply on real gas we can see that as we compress the gas it is compressible till a particular limit after that the gas is not further more compressible.