The final temperature of the lead-water system will be lower than the final temperature of the copper-water system.
<span>100.
ppb of chcl3 in drinking water means 100 g of CHCl3 in 1,000,0000,000 g of water
Molarity, M
M = number of moles of solute / volume of solution in liters
number of moles of solute = mass of CHCl3 / molar mass of CHCl3
molar mass of CHCl3 = 119.37 g/mol
number of moles of solute = 100 g / 119.37 g/mol = 0.838 mol
using density of water = 1 g/ ml => 1,000,000,000 g = 1,000,000 liters
M = 0.838 / 1,000,000 = 8.38 * 10^ - 7 M <----- answer
Molality, m
m = number of moles of solute / kg of solvent
number of moles of solute = 0.838
kg of solvent = kg of water = 1,000,000 kg
m = 0.838 moles / 1,000,000 kg = 8.38 * 10^ - 7 m <----- answer
mole fraction of solute, X solute
X solute = number of moles of solute / number of moles of solution
number of moles of solute = 0.838
number of moles of solution = number of moles of solute + number of moles of solvent
number of moles of solvent = mass of water / molar mass of water = 1,000,000,000 g / 18.01528 g/mol = 55,508,435 moles
number of moles of solution = 0.838 moles + 55,508,435 moles = 55,508,436 moles
X solute = 0.838 / 55,508,435 = 1.51 * 10 ^ - 8 <------ answer
mass percent, %
% = (mass of solute / mass of solution) * 100 = (100g / 1,000,000,100 g) * 100 =
% = 10 ^ - 6 % <------- answer
</span>
42,256 = 2,000
42,256 = 200
together they'd be 2,200 (if that's what you needed as well)
25 g of NH₃ will produce 47.8 g of (NH₄)₂S
<u>Explanation:</u>
2 NH₃ + H₂S ----> (NH₄)₂S
Molecular weight of NH₃ = 17 g/mol
Molecular weight of (NH₄)₂S = 68 g/mol
According to the balanced reaction:
2 X 17 g of NH₃ produces 68 g of (NH₄)₂S
1 g of NH₃ will produce
g of (NH₄)₂S
25g of NH₃ will produce
of (NH₄)₂S
= 47.8 g of (NH₄)₂S
Therefore, 25 g of NH₃ will produce 47.8 g of (NH₄)₂S
Answer:
i) Highest osmotic pressure: CaCl2
ii) lower vapor pressure : CaCl2
iii) highest boiling point : CaCl2
Explanation:
The colligative properties depend upon the number of solute particles in a solution.
The following four are the colligative properties:
a) osmotic pressure : more the concentration of the solute, more the osmotic pressure
b) vapor pressure: more the concentration of the solute, lesser the vapor pressure.
c) elevation in boiling point: more the concentration of the solute, more the boiling point.
d) depression in freezing point: more the concentration of the solute, lesser the freezing point.
the number of particle produced by urea = 1
the number of particle produced by AgNO3 = 2
the number of particle produced by CaCl2 = 3
As concentrations are same, CaCl2 will have more number of solute particles and urea will have least
i) Highest osmotic pressure: CaCl2
ii) lower vapor pressure : CaCl2
iii) highest boiling point : CaCl2