What are some reasons why you don't get a 100 percentage yield from a reaction?
What are some reasons why you don't get a 100 percentage yield from a reaction? Chemistry homework. I need 5 reasons! % yield = 100 * (Actual amount) / (Expected amount) In real life, substances are not 100 % pure. This means the mass of reactants is less than the measured amount of reactants. The mathematical expected amount is larger than it should be. The impurities do not yield the desired products, so the yield is less than 100%. Improper measurements can make the make the answers less or more than reality. The ratio of the moles of reactants to moles of products is determined by the coefficients in the balanced equation. If you do not have exactly the correct amount of each reactant, the reaction will not yield the expected amount of products. This is called limiting factor. Many reactions require energy, such as heat or electricity to react. If the heat is removed or the electricity turned off before the reaction is complete, the yield will be less than the expected amount. And When heating a crucible or test tube, some the chemical get ejected out of the container. This is fun to watch! But the result is poor yield!
You don't need a reason to help people . what is the meaning of this phrase?
You help people because it's the right thing to do and it makes others feel good, you don't need to receive anything in return for helping them.