Answer: 2.39 atm 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 Log in to Reply

Answer:

2.39 atm

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