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

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.