If green spheres represent chlorine atoms and red spheres...

If green spheres represent chlorine atoms and red spheres represent oxygen atoms, $(7.1,7.8)$
a. Write a balanced equation for the reaction.
b. identify the limiting reactant.
c. from the diagram of the actual products that result, calculate the percent yield for the reaction.

Key Concepts

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of the product obtained experimentally to the theoretical yield predicted by stoichiometry. The calculation provides insights into the practical aspects of the reaction, including potential losses or side reactions that might have occurred during the experiment.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first during a reaction, thereby limiting the amount of product that can be formed. Identifying the limiting reactant is crucial for determining the theoretical yield and quantitatively analyzing the overall efficiency of the reaction.

Balanced Chemical Equation

A balanced chemical equation represents the reaction by showing equal numbers of each type of atom on both sides of the equation, which demonstrates the conservation of mass. It involves adjusting stoichiometric coefficients so that the number of atoms for each element is the same in the reactants and products, ensuring accurate quantitative predictions in chemical reactions.

Transcript

00:01 This question has three parts.

00:02 So the first part asks us to write a balanced equation for the reaction.

00:06 So our reactants are diatomic green molecules, which are chlorines, and diatomic red molecules, which are oxygens.

00:17 Our products are going to be three atom molecules, consisting of one red, which is oxygen, and two chlorines, green molecules.

00:30 All right.

00:32 So what's our equation going to look like? well, cl2 plus o2 forms ocl2.

00:42 Now the question is, is this balanced? well, we see that it is not, because we have two oxygens on the left, but only one on the right.

00:50 So what do we do? put a coefficient of two in front of the o .c .l .2 in our products.

00:55 But now, although our oxygens are balanced, right, our chlorines are not.

01:03 Because we have four chlorines on the right and only two on the left.

01:06 So we'll put another coefficient of two.

01:08 In front of the chlorine on the left side, and now everything is balanced.

01:18 So this is our equation.

01:21 For part b, let's identify the limiting reactant.

01:25 Is it chlorine or is it oxygen? well, let's think about it, right? in our reactants, we had three, three of our reds, so three oxygens, but we had four chlorines.

01:40 All right.

01:42 But as you can see here, the ratio of reactants is, 2 to 1, meaning we need 2 chlorines for every 1 oxygen.

01:54 That's 2 to 1.

01:59 As we can see here, if we have 3 oxygens, that means we would expect 6 chlorines, 2 to 1 ratio.

02:14 So therefore, our chlorines are the limiting.

02:25 Cl2 is the limiting...

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