69.1k views
1 vote
0.41g of neon is held in a 200. mL container at 11 °C. Calculate the pressure in atm.

1 Answer

2 votes

Answer:

2.39 atm

Step-by-step explanation:

We'll begin by calculating the number of mole in 0.41 g of neon (Ne). This can be obtained as follow:

Mass of Ne = 0.41 g

Molar mass of Ne = 20 g/mol

Mole of Ne =.?

Mole = mass / molar mass

Mole of Ne = 0.41 / 20

Mole of Ne = 0.0205 mole

Next we shall convert 200 mL to L.

1000 mL = 1 L

Therefore,

200 mL = 200 mL × 1 L / 1000 mL

200 mL = 0.2 L

Next, we shall convert 11 °C to Kelvin temperature.

T(K) = T(°C) + 273

T(°C) = 11 °C

T(K) = 11 + 273

T (K) = 284 K

Finally, we shall determine the pressure. This can be obtained as follow:

Mole of Ne (n) = 0.0205 mole

Volume (V) = 0.2 L

Temperature (T) = 284 K

Gas constant (R) = 0.0821 atm.L/Kmol

Pressure (P) =?

PV = nRT

P × 0.2 = 0.0205 × 0.0821 × 284

P × 0.2 = 0.4779862

Divide both side by 0.2

P = 0.4779862 / 0.2

P = 2.49 atm

Therefore, the pressure of the gas is 2.39 atm

User Jamie Carl
by
8.2k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.