Transcript
In chemical reactions, atoms — which are the building blocks of reactants — are rearranged to form new entities called products. The law of the conservation of masses states that matter can neither be created nor destroyed. Thus, for a chemical reaction in an isolated system, the mass remains constant.
The number of atoms on the reactant side equals that on the product side, and we see that the equation is balanced. This relationship between reactant and product quantities is known as stoichiometry.
Now, let's practice balancing a chemical equation. Here are the coefficients for carbon dioxide and nitrogen dioxide to help you get started. First, let's count the number of atoms on each side. Pay attention to both the coefficient, which indicates how many molecules are in the equation, and the subscript, which tells us how many atoms are in a molecule.
Then, multiply the coefficient and subscript values for each atom. Repeat for all elements. If an element is in several molecules, simply add the number of atoms in each molecule. Once this is complete for all elements, check to see if the reaction is balanced.
At its current state, the equation is not balanced. We see that there is one nitrogen on the reactant side, but four on the product side. To balance nitrogen, we need four reactant molecules, so we multiply all its elements by four. This balances carbon as well. There are two hydrogen atoms on the product side. Thus, we will make 14 H2O products. This makes 38 oxygen atoms on the product side, which requires 19 oxygen molecules on the reactant side. Finally, the equation is balanced.
The relationship between coefficients represents the relationship between the molar amounts. In this equation, one molecule of methane reacts with two molecules of oxygen to make one molecule of carbon dioxide and two molecules of water. The reaction stops when any reactant is completely consumed, limiting the amount of product that can be made. That reactant is called the limiting reactant.
The maximum possible amount of product, which is called the theoretical yield, depends on the amount of the limiting reactant. However, the actual product yield may differ based on side reactions, loss from purification steps, or human error. The percent yield tells us what percentage of the theoretical yield was obtained and is determined with this equation.
In this lab, you will react nickel chloride hexahydrate with ethylenediamine to synthesize a nickel coordination complex. Then, you will measure the amount produced, determine the limiting reactant of the reaction, and calculate the percent yield of the product.
Abstract
Chemical equations represent how a chemical reaction proceeds from reactants to products through physical or chemical change using chemical formulas.
Stoichiometry is a term that describes the relative quantities of reactants and products in a chemical reaction. It is based on the Law of Conservation of Mass, which is a fundamental law that states that matter is neither created nor destroyed. Quite simply, the number and identity of reactant atoms must equal the number and identity of product atoms. Reactions rearrange atoms but do not create or destroy them. This requires that a proposed reaction must be balanced, meaning that the number of atoms for each element are equal on the reactant and product sides.
For example, in the chemical equation below, the left side (the reactants) includes one copper atom, one hydrogen atom, one nitrogen atom, and three oxygen atoms.
Cu + HNO3 → Cu(NO3)2 + 4 H2O + NO
On the right side, notice the water product has a number preceding it. This is a coefficient and represents the number of molecules in the reaction. Using this information, we can tally the number of atoms on the product side. There is one copper atom and eight hydrogen atoms (4 x 2). Tallying the nitrogen and oxygen atoms requires a bit more math. There are two nitrogen atoms in the first product and one nitrogen atom in the third product, which gives a total of three nitrogen atoms. For oxygen, there are six oxygen atoms in the first product, four oxygen atoms in the second product, and one oxygen atom in the third product for a total of 11 oxygen atoms.
If left in this form, the reaction wouldn’t be feasible because it defies the Law of Conservation of Masses. There are more hydrogen, nitrogen, and oxygen atoms on the product side. Therefore, the equation needs to be balanced.
Balancing an equation is an iterative process that requires adding coefficients to each side until the numbers become equal. There are several approaches to balance a chemical equation. One approach uses a table to visualize the numbers and a bit of trial and error.
| # of atoms on the reactant side | # of atoms on the product side | ||||||
| Copper | Hydrogen | Nitrogen | Oxygen | Copper | Hydrogen | Nitrogen | Oxygen |
| 1 | 1 | 1 | 3 | 1 | 8 | 3 | 11 |
Since there is only one hydrogen atom on the reactant side but eight hydrogen atoms on the product side, multiplying the compound containing the nitrogen on the reactant side by eight would balance hydrogen. The second row in the new table reflects this change to the number of atoms.
| # of atoms on the reactant side | # of atoms on the product side | |||||||
| Copper | Hydrogen | Nitrogen | Oxygen | Copper | Hydrogen | Nitrogen | Oxygen | |
| 1 | 1 | 1 | 3 | 1 | 8 | 3 | 11 | |
| 8 HNO3 | 1 | 8 | 8 | 24 | 1 | 8 | 3 | 11 |
Next, to increase the number of nitrogens on the product side, multiplying the product Cu(NO3)2 by three would raise the number of nitrogen atoms from three to seven. The number of nitrogen atoms is not balanced yet, but there are still coefficients for one reactant and one product to consider.
| # of atoms on the reactant side | # of atoms on the product side | |||||||
| Copper | Hydrogen | Nitrogen | Oxygen | Copper | Hydrogen | Nitrogen | Oxygen | |
| 1 | 1 | 1 | 3 | 1 | 8 | 3 | 11 | |
| 8 HNO3 | 1 | 8 | 8 | 24 | 1 | 8 | 3 | 11 |
| 3 Cu(NO3)2 | 1 | 8 | 8 | 24 | 3 | 8 | 7 | 23 |
If there are two molecules of NO produced, this adds one more nitrogen atom and one more oxygen atom to the product side, balancing these two species with the reactant side.
| # of atoms on the reactant side | # of atoms on the product side | |||||||
| Copper | Hydrogen | Nitrogen | Oxygen | Copper | Hydrogen | Nitrogen | Oxygen | |
| 1 | 1 | 1 | 3 | 1 | 8 | 3 | 11 | |
| 8 HNO3 | 1 | 8 | 8 | 24 | 1 | 8 | 3 | 11 |
| 3 Cu(NO3)2 | 1 | 8 | 8 | 24 | 3 | 8 | 7 | 23 |
| 2 NO | 1 | 8 | 8 | 24 | 3 | 8 | 8 | 24 |
The only atom left unbalanced now is copper. Increasing the number to three copper atoms on the reactant side balances the equation.
| # of atomson the reactant side | # of atoms on the product side | |||||||
| Copper | Hydrogen | Nitrogen | Oxygen | Copper | Hydrogen | Nitrogen | Oxygen | |
| 1 | 1 | 1 | 3 | 1 | 8 | 3 | 11 | |
| 8 HNO3 | 1 | 8 | 8 | 24 | 1 | 8 | 3 | 11 |
| 3 Cu(NO3)2 | 1 | 8 | 8 | 24 | 3 | 8 | 7 | 23 |
| 2 NO | 1 | 8 | 8 | 24 | 3 | 8 | 8 | 24 |
| 3 Cu | 3 | 8 | 8 | 24 | 3 | 8 | 8 | 24 |
The balanced equation is written as follows:
3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 4 H2O + 2 NO
Balancing the equation is also essential for determining the limiting reactant because the coefficient of the compounds is used to calculate how much product is produced by each reactant (product yield). From this quantity, the reactant producing the least amount of product is considered the limiting reactant--which is completely consumed in the reaction and therefore limits the total amount of product generated. This calculated quantity also represents the theoretical yield of the reaction, which is needed to calculate the percent yield.
The balanced equation is more than a simple accounting of atoms. The coefficients describe the molar relationship between products and reactants, i.e., how much product is produced by each reactant. The number of moles of reactant is used to calculate the number of moles of another product or reactant. The reactant that produces the least amount of product is considered the limiting reactant.
The limiting reactant is completely consumed in the reaction and therefore limits the total amount of product generated. Once the limiting reactant is entirely consumed, no more product will form. The possible amount of product that could be formed based on the limiting reactant is the theoretical yield of the reaction.
The actual yield is compared to the theoretical yield, resulting in the ‘percent yield’. A percent yield of 100% means that, based on the reactants used, the maximum possible amount of product was produced. Percent yields less than 100% are common and indicate that there was some product loss during the reaction. The percent yield is never greater than the theoretical yield. If this is the case, experimental or calculation errors occurred.