Question

At 20°C the vapor pressure of dry ice is 56.5 atm. If 10g of dry ice (solid CO2) is placed in an evacuated 0.25 L chamber at a constant 20°C, will all of the solid sublime?

Answer 1

Answer:

All the solid CO2 (dry ice) will sublime

Explanation:

PV = nRT

Where P = pressure

V = volume

n = number of moles

R = universal gas constant

T = temperature

Given values.

P = 56.5_atm =5.72_MPa

V = 0.25_L

n = Unknown

R = 8.31451_j/(gmol×K)

T = (273.15 + 20) = 293.15_K

Thus, n, from the above equation = (P×V) ÷ (R×T)

= 1431.216 ÷ 2437.399÷ = 0.587_moles

Molar mass of CO2 = 44_g

Number of moles in 10_g of CO2 = 10/44 = 0.23 moles

0.23 moles < 0.587_moles hence the volume has capacity for 0.36_moles of CO2 more

All the solid CO2 (dry ice) will sublime

Answer 2

All the solid CO2 will sublime in the evacuated chamber.

The given parameters:

• Temperature of the dry ice, T = 20°C  = 293 K.
• Vapor pressure of the dry ice, P = 56.5 atm
• Mass of the dry ice, m = 10g
• Volume of the ice, V = 0.25 L

The number of moles of the CO2 is the chamber is calculated using ideal gas law;

PV = nRT

$n = \frac{PV}{RT} \\\\n = \frac{56.5 \times 0.25}{0.0821 \times 293} \\\\ n = 0.587 \ mol$

The number of moles of 10g of solid CO2 is calculated as follows;

$n = \frac{10}{44} = 0.23 \ mol$

The chamber can accommodate more moles of CO2 than the current mass of CO2 placed in it.

Thus, all the solid CO2 will sublime in the evacuated chamber.

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