Question

A piece of solid carbon dioxide with a mass of 5.50 grams is placed in a 10 Liter vessel that already contains 705 torr at 24 Celsius. After the carbon dioxide has totally vaporized what is the partial pressure in the container at 24 Celsius?

Answer 1

total pressure = ( 705 torr + 231.525torr)  =   936.525torr

Answer 2

Answer:

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the quantity of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

The partial pressure of a gas is the pressure it exerts on a gas mixture.

The partial pressure for CO₂ is calculated using the ideal gas equation.

In this case, you initially have:

• P=?
• V=10 L
• $n=5.50 g*\frac{1molCO_{2} }{44 g CO_{2} } =0.125 moles CO_{2}$
• $R=62.364 \frac{torr*L}{mol*K}$
• T=24°C+273°K=297°K

Then  the partial pressure of CO₂ is:

$P=\frac{n*R*T}{V}$

$P=\frac{0.125 mol*62.364\frac{Torr*L}{mol*K} *297 K}{10 L}$

P≅231.53 torr

The total pressure of the mixture is the sum of the partial pressures that each gas contains. In this case the gases contained are air, with a pressure of 705 torr, and CO₂, with a pressure of 231.53 torr. So:

PT=Pair+PCO₂

PT=705 torr + 231.53 torr

PT=936.53 torr