Question

At what temperature celsius will 19.4g of molecular oxygen, o2, exert a pressure of 1820mm hg in a 5.12th cylinder?

Answer 1

T = -28.2 °C

Step-by-step explanation:

Answer 2

Answer:
T = -28.2 °C

Solution:

Data Given;
P = 1820 mmHg = 2.39 atm

V = 5.12 L

m = 19.4 g

R = 0.0821 atm.L.mol⁻¹.K⁻¹

Calculating moles,

n = 19.4 g ÷ 32 g.mol⁻¹

n = 0.606 mol

Assuming that the oxygen gas is acting perfectly, then according to Ideal Gas Equation,
P V = n R T

Solving for T,
T = P V / n R

Putting values,

T = (2.39 atm × 5.12 L) ÷ (0.606 mol × 0.0821 atm.L.mol⁻¹.K⁻¹)

T = 244.7 K
Or,
T = -28.2 °C