Q-8 Determine the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively.?
Answer :- .
| Elements | Symbol | % by mass | atomic mass | % by mass/atomic mass | simple ratio | simple whole number ratio |
| Iron | Fe | 69.9 | 55.85 | 69.9/55.85 = 1.25 | 1.25/1.25=1(divide by smaller number of privious coloumn) | 2(multiply by 2 to change in whole number ) |
| Oxygen | O | 30.1 | 16.00 | 30.1/16.00 =1.88 | 1.88/1.25=1.5 | 3 |
imperical formula = Fe2O3
hence molecular formula is same as empirical formula Fe2O3
how do we know the mass of unknown oxide of iron???
ReplyDeleteplease type your complete problem
ReplyDeletewe can know the molar mass by mass percent
ReplyDeletefe is 69.9% therefore. (55.85/molar mass)x100 =69.9
molar mass comes equal to 159.7
we can know the molar mass by mass percent
ReplyDeletefe is 69.9% therefore. (55.85/molar mass)x100 =69.9
molar mass comes equal to 159.7
we can know the molar mass by mass percent
ReplyDeletefe is 69.9% therefore. (55.85/molar mass)x100 =69.9
molar mass comes equal to 159.7
(55.85/69.9)100=molar mass =79.899
ReplyDeletesir who we calculated molar mass in calculating multiplying factor
ReplyDeleteCalculate the concentration of nitric acid in moles per lit in a sample which has density 1.41 gm/L and mass percentage of nitric acid in it being 69%
ReplyDeleteCalculate the concentration of nitric acid in moles per lit in a sample which has density 1.41 gm/L and mass percentage of nitric acid in it being 69%
ReplyDelete