Answer:
0.998 atm.
Step-by-step explanation:
NOTE: The temperature is missing in the above question and the value is 20 °C
From the question given above, the following data were obtained:
Volume (V) = 10.0 L
Number of mole of H₂ = 0.2 mole
Number of mole N₂ = 0.215 mole
Temperature (T) = 20 °C
Total pressure (P) =?
Next, we shall determine the total number of mole in flask. This can be obtained as follow:
Number of mole of H₂ = 0.2 mole
Number of mole of N₂ = 0.215 mole
Total number of mole (n) =?
n = mole of H₂ + mole of N₂
n = 0.2 + 0.215
n = 0.415 mole
Thus, the total number of mole in the flask is 0.415 mole
Next, we shall convert 20 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Temperature (T) = 20 °C + 273
Temperature (T) = 293 K
Finally, we shall determine the total pressure in the flask. This can be obtained as follow:
Volume (V) = 10.0 L
Total number of mole (n) = 0.415 mole
Temperature (T) = 293 K
Gas constant (R) = 0.0821 atm.L/Kmol
Total pressure (P) =?
PV = nRT
P × 10 = 0.415 × 0.0821 × 293
Divide both side by 10
P = (0.415 × 0.0821 × 293) / 10
P = 0.998 atm.
Therefore, the total pressure in the flask is 0.998 atm.