Rank the following samples according to increasing mass of oxygen from lowest to highest.?

Question

A. 35.0 g CO2
B. 10.0 g SO2
C. 20.0 g Fe(NO3)2
D. 18.0 g CH3OH

Answer 1

To solve this problem, first find the percent composition (by mass) of Oxygen in the compound by dividing the mass of Oxygen in the compound by the molar mass of the compound.
Then, after you have found the % composition of Oxygen, multiply by the mass of the sample you have to find the mass of the Oxygen present in the sample of the compound.

Carbon Dioxide:
Molar mass of CO2 = 44.01 g/mol
Mass of Oxygen = 32 g/mol.
% Oxygen = 72.7%
Mass of Oxygen within 35.0 grams of CO2 = .727 * 35.0 grams = 25.4 grams Oxygen.

Sulfur Dioxide:
Molar mass of SO2 = 64.07 g/mol
Mass of Oxygen = 32 g/mol.
% Oxygen = 49.9%
Mass of Oxygen within 10.0 grams of SO2 = .499 * 10.0 grams = 4.99 grams Oxygen.

Iron (II) Nitrate
Molar mass of Fe(NO3)2 = 179.87 g/mol
Mass of Oxygen = 96 g/mol.
% Oxygen = 53.4%
Mass of Oxygen within 20.0 grams of Fe(NO3)2 = .534 * 20.0 grams = 10.7 grams Oxygen.

Methanol
Molar mass of CH3OH = 32.05 g/mol
Mass of Oxygen = 16 g/mol.
% Oxygen = 49.9%
Mass of Oxygen within 18.0 grams of CH3OH = .499 * 18.0 grams = 9.0 grams Oxygen.

So we can now order these values from greatest to least.
The Carbon Dioxide sample is first, then the Iron (II) Nitrate, then Methanol, and lastly Sulfur Dioxide, for the amounts listed.

Answer 2

4 hydroxy benzoic acid < benzoic acid < 4 methoxy phenol < cycloheptanol < trimethyl amine acidity ability for a typical compounds how plenty H+ ions are required to neutralize.