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

Answer:

The volume inside the balloon is = 121 $m^{3}$

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 $m^{3}$

Answer 2

Answer:

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

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

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