Calculate the pressure of 2.78 g of Ne in a 5.00 L flask at -10°C

0.60 atm

Explanation:

Step 1.

Data obtained from the question.

This includes the following:

Mass of Ne = 2.78g

Volume (V) = 5L

Temperature (T) = –10°C

Pressure (P) =?

Step 2:

Determination of the number of mole of Ne.

The number of mole of Ne can be obtained as follow:

Mass of Ne = 2.78g

Molar Mass of Ne = 20g/mol

Number of mole Ne =?

Number of mole = Mass/Molar Mass

Number of mole of Ne = 2.78/20

Number of mole of Ne = 0.139 mol

Step 3:

Conversion of celsius temperature to Kelvin temperature. This can be achieved by as shown below:

Temperature (Kelvin) = temperature (celsius) + 273

Temperature (celsius) = –10°C

Temperature (Kelvin) = –10°C + 273

Temperature (Kelvin) = 263K

Step 4:

Determination of the pressure. The pressure can be obtained by using the ideal gas equation as follow:

PV = nRT

Volume (V) = 5L

Temperature (T) = 263K

Number of mole (n) of Ne = 0.139mol

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

Pressure (P) =?

PV = nRT

P x 5 = 0.139 x 0.082 x 263

Divide both side by 5

P = (0.139 x 0.082 x 263) /5

P = 0.60 atm

Therefore the pressure is 0.60 atm

the answers would be

the first one and the second one

2b2t

explanation:

2b2t