Answer:
a number should be rounded up it is 5 or higher
Answer:
The gas was N₂
Explanation:
V = 3.6L
P = 2.0 atm
T = 24.0°C = 297K
R = 0.0821 L.atm/K.mol
m = 8.3g
M = molar mass = ?
Using ideal gas equation;
PV = nRT
n = no. Of moles = mass / molar mass
n = m/M
PV = m/M * RT
M = mRT / PV
M = (8.3*0.0821*297) / (2.0*3.6)
M = 28.10
Since X is a diatomic molecule
M = 28.10 / 2 = 14.05 g/mol
M = Nitrogen
X = N₂
Answer:
16.06 L was the initial volume of the balloon.
Explanation:
Initial moles of freon in ballon = 
Initial volume of freon gas in ballon = 
Moles of freon gas added in the balloon = n = 3.50 mole
Final moles of freon in ballon = 
Final volume of freon gas in ballon = 
Using Avogadro's law:
( at constant pressure and temperature)
16.06 L was the initial volume of the balloon.
First, we need the no.of moles of O2 = mass/molar mass of O2
= 55 g / 32 g/mol
= 1.72 mol
from the balanced equation of the reaction:
2H2 (g) + O2(g) → 2H2O(g)
we can see that the molar ratio between O2: H2O = 1: 2
So we can get the no.of moles of H2O = 2 * moles of O2
= 2 * 1.72 mol
= 3.44 mol
So by substitution by this value in ideal gas formula:
PV = nRT
when P = 12.4 atm & n H2O = 3.44 mol & R= 0.0821 & T = 85 + 273=358K
12.4 atm *V = 3.44 * 0.0821 * 358 = 8.15 L
∴ V ≈ 8.2 L
