18) Chlorine reacts with potassium bromide to produce potassium chloride and bromine.

A) write a chemical equation, using words, to represent the above chemical reaction.
My answer:
chlorine + potassium bromide ==> potassium chloride and bromine
( I'm pretty sure this is right)

B) Suppose 4.0 g of chlorine complete reacts with 13.4 g of potassium bromide producing 8.4 g of potassium chloride. What mass of bromine is produced?

(HOW DO I DO THIS ONE)

My attempted answer: 4.0 g chlorine + 13.4 g potassium chloride ==> 17.4 bromine??

On tge first question I suggest you change the arrow to a word; i.e., yields or produces or gives. Yields is the best one to use I think. I would also change the + sign to a word like "and" or write the word "plus" there. I prefer plus.

For the second one, I will write the equation with symbols and the solution undr it. Your answer is on the right track but isn't correct. Remember the law of conservation of mass. It must add up on both sides to the same.
........Cl2 + 2KBr ==> 2KCl + Br2
.......4.0.....13.4.....8.4....?
So 13.4 + 4.0 = 13.4 + ?
And solve for ?

damn if i know

To determine the mass of bromine produced in the reaction, we need to use the law of conservation of mass. This law states that the total mass of the reactants must be equal to the total mass of the products.

First, we need to calculate the molar masses of the substances involved:
- Chlorine (Cl2) has a molar mass of 35.45 g/mol.
- Potassium bromide (KBr) has a molar mass of 119 g/mol.
- Potassium chloride (KCl) has a molar mass of 74.55 g/mol.

Next, we can use the balanced chemical equation to determine the mole ratios:
1 mole of chlorine reacts with 1 mole of potassium bromide to produce 1 mole of potassium chloride and 1 mole of bromine.

Now, let's calculate the number of moles for each substance:
- Moles of chlorine = mass of chlorine / molar mass of chlorine = 4.0 g / 35.45 g/mol = 0.113 mol (rounded to 3 decimal places)
- Moles of potassium bromide = mass of potassium bromide / molar mass of potassium bromide = 13.4 g / 119 g/mol = 0.112 mol (rounded to 3 decimal places)
Since the reaction is based on mole ratios, we can see that chlorine and potassium bromide have similar moles, which means chlorine is the limiting reactant.

Now, let's use the mole ratio to determine the moles of bromine produced:
- Moles of bromine = moles of chlorine = 0.113 mol (rounded to 3 decimal places)

Finally, we can calculate the mass of bromine:
Mass of bromine = moles of bromine x molar mass of bromine = 0.113 mol x 79.90 g/mol = 9.067 g (rounded to 3 decimal places)

Therefore, the mass of bromine produced in the reaction is approximately 9.067 grams.

To solve part B, you need to use the concept of stoichiometry. Start by balancing the chemical equation:

Cl2 + 2KBr → 2KCl + Br2

Now we can establish the mole ratios between the reactants and products. From the balanced equation, we can see that for every 1 mole of chlorine (Cl2) reacted, 1 mole of bromine (Br2) is produced.

To calculate the moles of each substance, divide the given masses by their respective molar masses:

Moles of chlorine (Cl2) = 4.0 g / molar mass of Cl2
Moles of potassium bromide (KBr) = 13.4 g / molar mass of KBr
Moles of potassium chloride (KCl) = 8.4 g / molar mass of KCl

Since the molar mass of Cl2 is 70.91 g/mol, the molar mass of KBr is 119.0 g/mol, and the molar mass of KCl is 74.55 g/mol, we can substitute these values into the equations:

Moles of chlorine (Cl2) = 4.0 g / 70.91 g/mol
Moles of potassium bromide (KBr) = 13.4 g / 119.0 g/mol
Moles of potassium chloride (KCl) = 8.4 g / 74.55 g/mol

Now compare the mole ratios to determine the number of moles of bromine produced. From the balanced equation, we know that the mole ratio of Cl2 to Br2 is 1:1, so the amount of bromine produced will be the same as the amount of chlorine reacted.

Therefore, the moles of bromine produced = Moles of chlorine (Cl2)

Finally, to find the mass of bromine produced, multiply the moles of bromine by its molar mass:

Mass of bromine produced = Moles of bromine x molar mass of bromine

Plug in the values and calculate the mass of bromine.