Question

How many moles of co2 are there in a 50.0 dm3 sample of the gas at a pressure of 100.0 kpa and a temperature of 50°c?

Answer 1

1.86 moles

Step-by-step explanation:

The equation you need to use is PV = nRT, where n is the value you are searching for.

P = 100.0 kPA

V = 50.0 dm^3

n = ?

R = 8.314

T = 50 celsius converted to kelvin (323 k)

Multiply the pressure times the volume (100*50) and divide it by the constant (R) by the temperature (8.314*323).

(100*50) / (8.314*323) = 5000 / 2685.422 = 1.86 moles

Answer 2

• 609 mol

Step-by-step explanation:

1) Data:

a) n = ?

b) V = 50.0 dm³ = 50.0 liter

c) p = 100.0 kPa

d) T = 50 °C

2) Physical law:

• Ideal gas law: pV = nRT,

3) Constants:

• R = 0.08206 atm-liter / K-mol

4) Unit conversions:

• T = 50 + 273.15 K = 323.15 K

• P = 100.0 kPa × (1 amt /101,325 kPa) = 0.9869 atm

5) Solution:

• pV = nRT ⇒ n = pV / (RT)

• n = 0.9869 atm × 50.0 liter / (0.08206 atm-liter /K-mol × 323.15 K)

• n = 609 mol ← answer