Question

A 1.00 mole sample of gas occupies a volume of 400.00ml.If the amount of gas is increased to 2.50 moles at the same temperature and Pressure. What will the new volume be ?​

Answer 1

Answer:

1l

Explanation:

1mole=400ml

2.50mole = 400×2.50ml

=1000ml or 1l

Answer 2

Answer:

After the amount of gas increases, the new volume of the gas, V₂, calculated is $1000ml$.

Explanation:

Data given,

The number of moles of the sample of gas, n₁ = $1.00mole$

The volume of the sample of gas, V₁ = $400ml$

After the amount of gas increased;

The new value of the number of moles, n₂ = $2.50moles$

The new volume of the gas, V₂ =?

As we know from the ideal gas equation:

• $PV = nRT$

Here, P = Pressure, T = Temperature, R = Raydberg's constant

As given, pressure and temperature are constant.

Therefore,

• V $\alpha$ n

We can write this as:

• $\frac{V_{1} }{n_{1} } = \frac{V_{2} }{n_{2} }$

After putting the given values of volume, and moles in the equation, we get:

• $\frac{400}{1.00} = \frac{V_{2} }{2.50}$
• V₂ = $1000ml$

Hence, the new volume of the gas, V₂ = $1000ml$.