Answer:
Mass = 80.6 g
Explanation:
Given data:
Mass of N₂ consumed = ?
Mass of CaCN₂ formed = 265 g
Solution:
Chemical equation:
CaC₂ + N₂ → CaCN₂ + C
Number of moles of CaCN₂:
Number of moles = mass/molar mass
Number of moles = 265 g/ 92.11 g/mol
Number of moles = 2.88 mol
Now we will compare the moles of CaCN₂ and N₂.
CaCN₂ : N₂
1 : 1
2.88 : 2.88
Mass of N₂:
Mass = number of moles × molar mass
Mass = 2.88 mol × 28 g/mol
Mass = 80.6 g
Answer: 4.4 x 10^-7
Explanation:
0.000066 x 0.0000066 / 0.01
= 4.4 x 10^-7
Answer:
The final vapor pressure is 687.24mmHg
Explanation:
The clausius-clapeyron equation below will be used to solve this problem:
Where;
ΔH is heat of vaporization = 450 kJ/mol = 450000J/mol
initial vapor pressure P₁ = 400mmHg
initial temperature T₁ = 3030K
Final temperature T₂ = 3070K
R is ideal gas constant = 8.314 J/molK
final vapor pressure P₂ = ?
P₂/400 = 1.7181
P₂ = (400*1.7181)mmHg
P₂ = 687.24mmHg
The final vapor pressure is 687.24mmHg
An unsaturated solution is a chemical solution in which the solute concentration is lower than its equilibrium solubility.