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