If 45.6 g of CO2 is in a 2.75 L container at 25.0 °C, predict the pressure in this container, in kPa.

936.97 KPa

Explanation:

We'll begin by calculating the number of mole in 45.6 g of CO₂. This can be obtained as follow:

Mass of CO₂ = 45.6 g

Molar mass of CO₂ = 12 + (16×2)

= 12 + 32

= 44 g/mole

Mole of CO₂ =?

Mole = mass /molar mass

Mole of CO₂ = 45.6 / 44

Mole of CO₂ = 1.04 mole

Next, we shall convert 25.0 °C to Kelvin temperature. This can be obtained as follow:

T (K) = T (°C) + 273

T (°C) = 25.0 °C

T (K) = 25.0 °C + 273

T (K) = 298 K

Finally, we shall determine the pressure. This can be obtained as follow:

Mole of CO₂ (n) = 1.04 mole

Volume (V) = 2.75 L

Temperature (T) = 298 K

Gas constant = 8.314 KPa.L/Kmol

Pressure (P) =?

PV = nRT

P × 2.75 = 1.04 × 8.314 × 298

P × 2.75 = 2576.67488

Divide both side by 2.75

P = 2576.67488 / 2.75

P = 936.97 KPa

Thus, the pressure is 936.97 KPa

3 hours because it is a decent distance.