Examples of percent yield in the following topics:
-
- The percent yield of a reaction measures the reaction's efficiency.
- Then, percent yield can be calculated.
- If 18.0 grams were actually produced, the percent yield could be calculated:
- It also shows how to calculate the limiting reactant and the percent yield in a chemical reaction.
- Calculate the percent yield of a reaction, distinguishing from theoretical and actual yield.
-
- In addition, stoichiometry can be used to find quantities such as the amount of products that can be produced with a given amount of reactants and percent yield.
-
- It can be used to find the quantities of the products from given reactants in a balanced chemical reaction, as well as percent yield.
- Calculate concentrations of solutions in molarity, molality, mole fraction and percent by mass and volume.
-
- At standard temperature and pressure, hydrogen gas consists of 75 percent orthohydrogen and 25 percent parahydrogen.
- Hydrogen gas (H2) is highly flammable and will burn in air at a very wide range of concentrations between 4 percent and 75 percent by volume.
- Hydrogen gas can also explode in a mixture of chlorine (from 5 to 95 percent).
- Oxidation of hydrogen removes its electron and yields the H+ ion.
- Hydrogen naturally exists as three isotopes, denoted 1H, 2H, and 3H. 1H occurs at 99.98 percent abundance and has the formal name protium. 2H is known as deuterium and contains one electron, one proton, and one neutron (mass number = 2).
-
- If you have actually done this in the laboratory, you will know it is highly unlikely that the second trial will yield the same result as the first.
-
- As the equilibrium constant approaches zero, the reaction tends to form 100 percent reactants.
- As the equilibrium constant approaches infinity, the reaction tends to form 100 percent products.
- The equilibrium constant K = 1 states that there will be 50 percent products and 50 percent reactants.
- Smaller Ka values yield larger pKa values.
-
- Percent dissociation is symbolized by the Greek letter alpha, α, and it can range from 0%< α < 100%.
- To determine percent dissociation, we first need to solve for the concentration of H+.
- As we would expect for a weak acid, the percent dissociation is quite small.
- However, for some weak acids, the percent dissociation can be higher—upwards of 10% or more.
- Calculate percent dissociation for weak acids from their Ka values and a given concentration.
-
- Butane's percent composition can be calculated as follows:
- Mass percent H in butane: $\frac{10.079\:g\:H}{58.123\:g\:butane} \cdot 100$ = 17.3% H
- Mass percent C in butane: $\frac {48.044\:g \:C}{ 58.123 \:g \:butane} \cdot 100$ = 82.7% C
- This video shows how to calculate the percent composition of a compound.
- Translate between a molecular formula of a compound and its percent composition by mass
-
- Traditional medications such as chloroquine are effective in only 50 percent of patients where the parasite is drug-resistant.
- The vicinal glycols prepared by alkene hydroxylation (reaction with osmium tetroxide or permanganate) are cleaved to aldehydes and ketones in high yield by the action of lead tetraacetate (Pb(OAc)4) or periodic acid (HIO4).
- This oxidative cleavage of a carbon-carbon single bond provides a two-step, high-yield alternative to ozonolysis, that is often preferred for small scale work involving precious compounds.
-
- Ozone depletion describes two distinct but related phenomena observed since the late 1970s: (1) a steady decline of about 4 percent per decade in the total volume of ozone in Earth's stratosphere (the ozone layer); and (2) a much larger springtime decrease in stratospheric ozone over Earth's polar regions.
- The chlorine monoxide can then react with a second molecule of ozone (O3) to yield another chlorine atom and two molecules of oxygen.