A 5.50 gram sample of c2h6 gas has a volume of 2.50l. If the sample is at 41.2c what will it's pressure be?

1.89 atm

Explanation:

Step 1:

Data obtained from the question. This is shown:

Mass of C2H6 = 5.50 g

Volume (V) = 2.50 L

Temperature (T) = 41.2°C

Pressure (P) = ?

Step 2:

Conversion of celsius temperature to Kelvin temperature. This is illustrated below:

K = °C + 273

°C = 41.2°C

K = °C + 273

K = 41.2°C + 273

K = 314.2 K

Therefore the temperature is 314.2 K

Step 3:

Determination of the number of mole of C2H6. This is illustrated below:

Molar Mass of C2H6 = (12x2) + (6x1) = 24 + 6 = 30g/mol

Mass of C2H6 = 5.50 g

Number of mole of C2H6 = ? Number of mole = Mass / Molar Mass

Number of mole of C2H6 = 5.5/30

Number of mole of C2H6 = 0.183mol

Step 4:

Determination of the pressure.

The pressure can be obtained by applying the ideal gas equation as illustrated below:

PV = nRT

P=?

V = 2.50 L

T = 314.2 K

The number of mole (n) = 0.183mol

Gas constant (R) = 0.082atm. L/Kmol

PV = nRT

P x 2.5 = 0.183 x 0.082 x 314.2

Divide both side by 2.5

P = (0.183 x 0.082 x 314.2) / 2.5

P = 1.89 atm

Therefore, the pressure of the C2H6 is 1.89 atm