Reactions
The _____ are on the right side of the arrow in a chemical reaction, whereas _____ are on the left side of the arrow in a chemical reaction.
What does the law of conservation of state?
To get the same amount of each type of atom on both sides of the chemical equation.
If you have a mole of of paper clips, you would have _____ paper clips.
602 hexillion
If you see symbols such as (s), (g), (l), and (aq), these are refer to ______.
List what each one stands for.
States of matter
(s) - solid
(g) - gas
(l) - liquid
(aq) - aqueous (dissolved in a liquid solution)
Based on the law of conservation of mass, we can state what equation?
mass of reactants = mass of products
Why do we need to get the same number of both types of atoms on a chemical equation?
This will allow it to follow the law of mass of conservation, which all chemical reactions are supposed to follow.
When relating two quantities, we can record that ratio as fractions (sometimes called conversions). Write the possible fractions of the following ratio:
2 moles O2= 3 moles H2O
(Record your answer on a sheet of paper)
(2 moles O2) / (3 moles H2O)
OR
(3 moles H2O) / (2 moles O2)
Interpret the following chemical equation in words:
4Fe (s) + 3O2 (g) -> 2Fe2O3 (s)
iron will react with oxygen gas to produce iron oxide (or rust)
Alternatively,
4 moles of Fe will react with 3 moles of O2 to produce 2 moles of Fe2O3.
In a chemical reaction, 18g of reactants were used. How many grams of products were made? Why?
18 g of products were made. By the law of conservation of mass, the mass of the reactants (18g total) should be equal to mass of the products).
18 g reactant = x g products,
so there must be 18 g of product produced.
How can we manipulate both sides of the chemical equation to balance it?
We can change the coefficients of each substance or the number of copies used -- we CANNOT change the substance by changing the subscripts.
What is the molar mass of Mg(OH)2?
How would it be represented as a fraction?
1 mol Mg(OH)2 = 1 mol Mg + 2 mol O + 2 mol H
= 24 g/mol + 2(16 g/mol) + 2(1 g/mol)
= 58 g/mol
(58 g Mg(OH)2) / (1 mol Mg(OH)2)
OR
(1 mol Mg(OH)2) / (58 g Mg(OH)2)
What is the reactant in the following chemical equation?
__KClO3 -> __KCl + __O2
KClO3
A solid mass of 60 g is mixed with a solution weighing 30 g. A chemical reaction takes place and a gas is produced and is released into the environment. The mass of the remaining mixture is 70 g, what was the mass of the gas produced?
20 g of gas was produced and released into the environment.
Balance the following chemical equation:
__KClO3 -> __KCl + __O2
2KClO3 -> 2KCl + 3O2
For the following chemical equation:
4Fe (s) + 3O2 (g) -> 2Fe2O3 (s)
Say you has 15 moles of Fe, how many moles of Fe2O3 would be produced?
Show all work using dimensional analysis.
7.5 moles Fe2O3 (Will write out work)
What are the products of the chemical equation and what state of matter are those products in?
4Fe (s) + 3O2 (g) -> 2Fe2O3 (s)
Fe2O3 is the only product that is in the solid state.
Explain how you would calculate the exact weight of carbon dioxide (the gas) displaced from our law of conservation of mass lab. Your answer should include a discussion of the relevant products present in the balloon setup and how it differs when the balloon is removed. Reference the following chemical equation:
CH3COOH (aq) + NaHCO3(s) --> NaC2H3O2(aq) + H2O (l) + CO2 (g)
(You may draw visuals to illustrate your point)
When the reaction occurs, there is water produced, carbon dioxide produced, and a substance dissolved in water (aqueous). When the apparatus of the Erlenmeyer flask has the balloon over it, all three species are present after bubbles stop forming. The gas expands to fill the entire container except where the liquid is (which is the water and the NaC2H3O2 is dissolved in the solution). When the balloon is removed, the carbon dioxide is released into the environment leaving only the liquid with the dissolved NaC2H3O2.
Taking the difference of the apparatus with the balloon with the apparatus without the balloon will only give us the mass of the carbon dioxide.
Balance the following chemical equation:
__ C4H10 + __ O2 -> __ CO2 + __ H2O
2C4H10 + 13O2 -> 8CO2 + 10H2O
For the following chemical equation:
4Fe (s) + 3O2 (g) -> 2Fe2O3 (s)
Say you has 10 grams of Fe, how many grams of Fe2O3 would be produced?
Show all work using dimensional analysis.
There are 3 steps to this process:
1. grams of what you have -> moles of what you have
[You will use molar mass of the substance you have]
2. moles of what you have -> moles of what you need
[You will use the balanced chemical equation to relate the two quantities]
3. moles of what you need -> grams of what you need
[You will use molar mass of the substance you need]