Answer:
1.89 atm
Step-by-step 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