Answer:
ch20 is the empirical formula for glucose , c6h1206 is the molecular formula .
I believe that due to the rising heat the carbon dioxide will have despirced into the air
Answer:
Explanation:
Cu²⁺ + 2e⁻ → Cu ( copper gets reduced )
Cu → Cu²⁺ + 2e⁻ ( copper gets oxidized )
Oxidation:
Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.
Reduction:
Reduction involve the gain of electron and oxidation number is decreased.
Consider the following reactions.
4KI + 2CuCl₂ → 2CuI + I₂ + 4KCl
the oxidation state of copper is changed from +2 to +1 so copper get reduced.
CO + H₂O → CO₂ + H₂
the oxidation state of carbon is +2 on reactant side and on product side it becomes +4 so carbon get oxidized.
Na₂CO₃ + H₃PO₄ → Na₂HPO₄ + CO₂ + H₂O
The oxidation state of carbon on reactant side is +4. while on product side is also +4 so it neither oxidized nor reduced.
H₂S + 2NaOH → Na₂S + 2H₂O
The oxidation sate of sulfur is -2 on reactant side and in product side it is also -2 so it neither oxidized nor reduced.
B) The mass percentage of a solution is the ratio of the mass of solute to the mass of solvent expressed as a percentage. This becomes:
mass % = (NaCl mass) / (water mass) x 100
Mass % = 20 / 250 x 100
Mass % = 8%
C)
The molarity of a solution is the moles of solute present per liter of solution. The volume of the solution is:
250 mL = 0.25 L
Moles = mass / Mr
Moles = 20 / 58.44
Moles = 0.34
Molarity = moles / liter
Molarity = 0.34 / 0.25
Molarity = 1.36 M
Answer:
30.12 g/m is the molar mass of the compound
Explanation:
Freezing point depression to solve this. The formula for the colligative property is:
ΔT = Kf . m
ΔT = T° freezing pure solvent - T° freezing solution
Kf = Cryoscopic constant
m = molality (mol/kg)
T° freezing pure benzene: 5.5°C
(5.5°C - 1.02°C) = 5.12 °C/m . m
4.48°C = 5.12 °C/m . m
4.48°C / 5.12 °C/m = m → 0.875 mol/kg
Mol = mass / molar mas
Molality = mol /kg
Let's find out the molar mass, with this equation:
(6.59 g / Molar mass) / 0.250 kg = 0.875 mol/kg
6.59 g / molar mass = 0.875 mol/kg . 0.250 kg
6.59 g / molar mass = 0.21875 mol
6.59 g / 0.21875 mol = molar mass → 30.12 g/m
