What is the empirical formula of an oxide containing 49.5% manganese? (Hint: Oxide = compound of Mn with O). Mn O Mass of element (in g) (assuming 100 g of compound) 1._49.5_
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
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1.
What is the empirical formula of an oxide containing 49.5% manganese? (Hint: Oxide = compound of Mn with O).
| Mn | O | |
| Mass of element (in g) (assuming 100 g of compound) | 1._49.5_ | 2._50.5_ |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | Mn2O7 |
What is the empirical formula of strontium chloride in problem 5?
| Sr | Cl | |
| Mass of element (in g) | 1. 2.21 | 2. 1.79 |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | SrCl2 |
3.
What is the empirical formula of an compound containing 0.830 % H; 45.8% Mn; 53.4% O?
| H | Mn | O | |
| Mass of element (in g) (assuming 100 g of compound) | 1._0.830_ | 2._45.8__ | 3._53.4_ |
| Moles of element | 4.______ | 5.______ | 6.______ |
| Moles of element/Smallest moles | 7.______ | 8.______ | 9.______ |
| Multiplier | 10.______ | 10.______ | 10.______ |
| Empirical formula | HMnO4 |
4.
What is the empirical formula of an compound containing 81.8% C; 18.2% H.
| C | H | |
| Mass of element (in g) (assuming 100 g of compound) | 1._81.8_ | 2._18.2_ |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | C3H8 |
5.
8.00 g of iron when burned in air yields 11.44 g oxide. What is the empirical formula of this oxide?
| F e | O | |
| Mass of element (in g) | 1._8.00_ | 2._____ |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | F e2O3 |
6.
Given the empirical formula of NO2 and a molecular weight of 92.0 g/mol, what is the molecular formula?
MW of NO2= _____ (express in "g/mol NO2" and round to the nearest whole number).
MW of compound/MW of NO2= ____ (Round to the nearest whole number).
True formula of compound is N2O4
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