Question

A balloon is floating around outside your window. The temperature outside is -1 ∘C , and the air pressure is 0.700 atm . Your neighbor, who released the balloon, tells you that he filled it with 3.80 moles of gas. What is the volume of gas inside this balloon?

Answer 1

`\large \boxed{\text{121 L}}`

Step-by-step explanation:

We can use the Ideal Gas Law.

pV = nRT

Data:

p = 0.700 atm

n = 3.80 mol

T = -1 °C

Calculations:

1. Convert the temperature to kelvins

T = (-1 + 273.15) K= 272.15 K

2. Calculate the volume

`\begin{array}{rcl}pV &=& nRT\\\text{0.700 atm} * V & = & \text{3.80 mol} * \text{0.082 06 L}\cdot\text{atm}\cdot\text{K}^(-1)\text{mol}^(-1) * \text{272.15 K}\\0.700V & = & \text{84.86 L}\\V & = & \textbf{121 L} \\\end{array}\\\text{The volume of the balloon is $\large \boxed{\textbf{121 L}}$}`

Answer 2

The volume inside the balloon is = 121
`m^(3)`

Step-by-step explanation:

Temperature T = - 1 °c = 272 K

Pressure = 0.7 atm = 71 k pa

No. of moles = 3.8

Mass of the gas inside the volume = 3.8 × 4 = 15.2 kg

From ideal gas equation

P V = m R T

Put all the values in above formula we get

71 × V =15.2 × 2.077 × 272

V = 121
`m^(3)`

Therefore the volume inside the balloon is = 121
`m^(3)`