Chemical properties are mainly determined by the number of valence electrons (electrons which can be gained, lost, or shared) in the atom.
Answer: The molarity of solution is 0.453 M
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.
where,
n = moles of solute
= volume of solution in ml
moles of 
= 
Now put all the given values in the formula of molality, we get
Therefore, the molarity of solution is 0.453 M
Answer:
2.78 x 10⁻² M
Explanation:
Step 1:
Data obtained from the question.
Volume = 225mL / 1000 = 0.225L
Mass of K₂SO₃•8H₂O = 1.89g
Molarity =..?
Step 2:
Determination of the number of mole of K₂SO₃•8H₂O
This is illustrated below:
Mass of K₂SO₃•8H₂O = 1.89g
Molar mass of K₂SO₃•8H₂O = (39x2) + 32 + (16x3) + 8[(2x1) + 16] = 78 + 32 + 48 + 8[18] = 302g/mol
Number of mole = Mass/Molar Mass
Number of mole of K₂SO₃•8H₂O = 1.89/302 = 6.26x10⁻² mole
Step 3:
Determination of the molarity.
Molarity = mole /Volume
Molarity = 6.26x10⁻² /0.225
Molarity = 2.78 x 10⁻² M
Therefore, the molarity of the solution is 2.78 x 10⁻² M
Answer:
The partial pressure of hydrogen gas at equilibrium is 1.26 atm
Explanation:
Let's use the molar fraction to solve this:
Molar fraction = Moles of gas / Total moles
Molar fraction = Gas pressure / Total pressure
Without equilibrium, we can think that the total system pressure is the sum of the partial pressures of each gas.
1 atm N₂ + 2 atm H₂ = 3 atm
Molar fraction for H₂ = 2 atm / 3atm → 0.66
Let's replace the molar fraction in equilibrium
Gas pressure / 1.9 atm = 0.66
Gas pressure = 1.26atm
