Answer:
T₂ = 687.6 K
Explanation:
Given data:
Initial pressure = 108 Kpa = 108/101 = 1.06588 atm
Initial temperature = 20°C = 20+273.15 = 293.15 k
Final temperature = ?
Final pressure = 2.50 atm
Solution:
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
Now we will put the values in formula:
1.06588 atm / 293.15 K = 2.5 atm/T₂
T₂ = 2.5 atm ×293.15 K / 1.06588 atm
T₂ = 732.875 atm. K /1.06588 atm
T₂ = 687.6 K
Add the correct Coefficients to balance it out
Answer:
1083.6 g
Explanation:
At STP, 1 mol of any given mass will occupy 22.4 L.
With the information above in mind we can<u> calculate how many moles of nitrogen gas (N₂) are there in 867 L</u>:
- 867 L ÷ 22.4 L/mol = 38.7 mol
Finally we convert 38.7 moles of N₂ into grams, using its molar mass:
- 38.7 mol * 28 g/mol = 1083.6 g