A metal, M, forms an oxide having the formula M2O3 containing 52.92% metal by mass. Determine the atomic weight in g/mole of the metal (M). Please provide your answer in 2 decimal places.

26.98g/mol

Explanation:

The molar mass of M2O3 = 2M + 3O = 2M +(3x16) = 2M + 48

From the question, we were told that the mass percentage of M is 52.92%. This can be expressed below:

Mass of M/MM of oxide = 52.92%

2M / 2M + 48 = 52.92/ 100

Cross multiply to express in linear form

2M x 100 = 52.92(2M + 48)

200M = 105.84M + 2540.16

Collect like terms

200M — 105.84M = 2540.16

94.16M = 2540.16

Divide both side by 94.16, we have:

M = 2540.16 / 94.16

M = 26.98

The atomic weight of M is 26.98g/mol

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.