When Kb = 1.1 x 10^-6
∴ Ka = Kw / Kb
= 1.1 x 10^-14 / (1.1 x 10 ^-6)
= 1 x 10^-8
when the reaction equation when we assume the base is B
B + H2O ↔ BH+ + OH-
∴ Ka = [BH+][OH-]/[B]
1 x 10^-8 = X^2 / 0.49
X^2 = 4.9 x 10^-9
∴X = 7 x 10^-5
∴[OH-] = 7 x 10^-5
∴POH = -㏒[OH]
= -㏒7 x 10^-5
= 4.15
∴ PH = 14 - POH
14 - 4.15
= 9.85
We calculate first the number of moles of CO2 and H2O produced by dividing the given masses by the molar masses of CO2 and H2O.
moles CO2 = (12.9 g CO2) x (1 mole CO2 / 12 g CO2) = 1.075 moles.
moles H2O = (6.15 g H2O) x (1 mole H2O / 18 g H2O) = 0.36 moles
Then, we count the number of C, H, and O moles. This gives us 1.075 moles C, 2.5 moles O and 0.72 moles H. The empirical formula is,
C1.075H0.72O2.5
Simplifying,
C4H3O10
Since it is an ionic compound. it would be a good electrical conductor
Answer:
4804.5 g of SO₂ are needed to the reaction
Explanation:
The reaction to produce sulfuric acid is:
2SO₂ + O₂ + 2H₂O → 2H₂SO₄
Ratio is 1:2. 1 mol of oxygen needs 2 moles of sulfur dioxide in order to react. We can propose this rule of three.
If 1 mol of O₂ react to 2 moles of SO₂
Then, 37.50 moles of O₂ will react with (37.5 . 2) /1 = 75 moles of SO₂
We convert the moles to mass, to know the answer:
75 mol . 64.06 g / 1 mol = 4804.5 g of SO₂
Answer:
C) 11 g
Explanation:
first look to graph , you have x and y
x is mass of Fe
and y is mass of product
if the reaction consumes 2 g of Fe , ( look to x axis , look to 2 )
and go up until the black line touch the line of number 2
and go left and you will see the point become in the middle between 10 and 12
** 12 (11) 10 ***
Good Luck
