Answer:
The answer to the question is
The percentage yield when 500. g of SO₃ react with excess water to produce 575 g of H₂SO₄ is 81.63 %
Explanation:
The known variables are
Mass of SO₃ = 500 g
Mass of H₂SO₄ = 575 g
Molar mass of SO₃ = 80.0632 g/mol
Molar mass of H₂SO₄ = 98.079 g/mol
The reaction equation is
SO₃ +H₂O → H₂SO₄
One mole of SO₃ react with one mole of H₂O to produce one mole of H₂SO₄
Therefore number of moles of SO₃ in 500 g sample of SO₃ = (500 g)/(80.0632 g/mol) = 6.25 moles
Also number of moles of H₂SO₄ in 575 g sample of H₂SO₄ = (575 g)/(98.079 g/mol) = 5.86 moles
Which shows that the reaction is in the forward direction, production of H₂SO₄
Therefore 6.25 moles of SO₃ can produce 6.25 moles of H₂SO₄ and
The mass of 6.25 moles of H₂SO₄ = 6.25 moles × 98.079 g/mol = 612.51 g
Theoretical Yield = 612.51 g
Percentage Yield = 
= 
Percentage Yield = 81.63 %
Answer:
D. If the distance between the crests of the waves increase, the frequency decreases.
Explanation:
Wavelength is the distance between two successive crests and troughs while frequency is the number of complete cycle per seconds
Velocity = Frequency × wavelength
Frequency and wavelength are inversely proportion
Answer:
The empirical formula is same as the molecular formula = C6H10S2O
Explanation:
we start by dividing the percentage of each of the elements by their atomic mass
Carbon = 44.4/12 = 3.7
Hydrogen = 6.21/1 = 6.21
Sulphur = 39.5/32 = 1.234375
oxygen = 9.89/16 = 0.618125
That of oxygen is smallest so we divide all by that of oxygen
C = 3.7 / 0.618125 = 6
H = 6.21/ 0.618125 = 10
S = 1.234375/ 0.618125 = 2
Automatically, oxygen is 1
So the empirical formula is;
C6H10S2O
Let’s get its molecular formula. We multiply each of the subscript by the number;
(72 + 10 + 64 + 16)n= 162
162n = 162
n = 1
So the molecular formula is same as the empirical formula
Answer:
A mixture of two or more substances that are evenly mixed throughout.
Explanation:
This is because a solution shouldn't be chemically bonded, that's called a compound.
