The way you calculate the empirical formula is to firstly assume 100g. To find each elements moles you take each elements percentage listed, times it by one mole and divide it by its atomic mass. (ex: moles of K =55.3g x 1 mole/39.1g, therefore there is 1.41432225 moles of Potassium) Once you’ve completed this for every element you list each elements symbol beside it’s number of moles and divide by the smallest number because it can only go into its self once. After you’ve done this, you’ve found your empirical formula, which is the simplest whole number ratio of atoms in a compound. I’ve added an example of a empirical question I completed last semester :)
Answer:
(40 g O) / (15.99943 g O/mol) x (1 mol CaCO3 / 3 mol O) x (100.0875 g CaCO3/mol) =
83 g CaCO3
So answer D), although three significant digits are not justified.
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The liquid particles would have moved randomly because of the increase in thermal energy. They would move randomly and would be floating in the bottle moving randomly. The liquid would turn into gas form. Meaning that you would have water particles floating in the bottle moving randomly.
In an exothermic reaction heat is released by a chemical reaction. In an endothermic reaction heat is absorbed by a chemical reaction.
The reaction between ammonium nitrate and water absorbs heat from the surrounding environment. Endothermic Reaction
Three drops of concentrated sulfuric acid added to 100 milliliters of water in a beaker makes the beaker hot. Exothermic Reaction
Ammonium chloride dissolved in a beaker of water makes the beaker cold. Endothermic Reaction
Uranium atoms are split to produce nuclear energy. Exothermic Reaction
Water separates into hydrogen and oxygen when an electric current is run through it. Endothermic Reaction
Methane and oxygen are combined to produce methanol and heat. Exothermic Reaction
