Question

A reaction at 11.0°C evolves 133.mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1atm . Round your answer to 3 significant digits.

Answer 1

Answer:

V=3.10 L

Explanation:

Considering the ideal gas equation as:-

$PV=nRT$

where,  

P is the pressure = 1 atm

V is the volume = ?

n is the number of moles = 133 mmol = 0.133 mol

T is the temperature  

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (11.0 + 273.15) K = 284.15 K

R is Gas constant having value = 0.0821 L.atm/K.mol

So,  

$V=\frac{nRT}{P}$

Now by putting the values in the above equation

$V=\frac{0.133\times 0.0821\times 284.15}{1}$

V=3.10 L

Therefore the volume of the gas will be 3.10 L.