Answer:
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
