In determining the boiling point
of solutions, always take note of the number of ions that will dissociate in
the solution. It does not depend on the nature of the substance. The greater
the number of ions dissociated, the greater is the boiling point of the solution.
Answer:
Solution
1.4 gm of CaO⟶n0.4 gm of Oxygen
1.0 gm of O2⟶3.5 gm of Ca
According to the law of definite proportions
n/m=y/x
⇒1.4/0.4=3.5.
⇒3.5=3.5
Explanation:
Answer:
P(mixture) = 1.92 atm
Explanation:
Given data:
Mass of H₂ = 0.200 g
Mass of N₂ = 1.00 g
Mass of Ar = 0.820 g
Volume = 2 L
Temperature = 20°C
Pressure of mixture = ?
Solution:
Pressure of hydrogen:
Number of moles of hydrogen = mass / molar mass
Number of moles of hydrogen = 0.200 g / 2 g/mol
Number of moles of hydrogen = 0.1 mol
P = nRT / V
P = 0.1 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L
p = 2.41 atm. L /2 L
P = 1.2 atm
Pressure of nitrogen:
Number of moles of nitrogen = mass / molar mass
Number of moles of nitrogen = 1 g / 28 g/mol
Number of moles of nitrogen = 0.04 mol
P = nRT / V
P = 0.04 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L
p = 0.96 atm. L /2 L
P = 0.48 atm
Pressure of argon:
Number of moles of argon = mass / molar mass
Number of moles of argon = 0.820 g / 40 g/mol
Number of moles of argon = 0.02 mol
P = nRT / V
P = 0.02 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L
p = 0.48 atm. L /2 L
P = 0.24 atm
Total pressure of mixture:
P(mixture) = pressure of hydrogen + pressure of nitrogen + pressure of argon
P(mixture) = 1.2 atm + 0.48 atm + 0.24 atm
P(mixture) = 1.92 atm
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