How do you solve stoichiometry problems?

Question

I really don't understand how to solve these types of problems; if you have any website or information, it would really help.

Answer 1

The most important thing to remember is that a balanced equation and the coefficients of substances in the equation show you the relationships between moles of one thing and moles of any other. So, you can always use the coefficients to convert or to relate moles of any reactant to moles of another reactant or to moles of a product.

Usually, though, you'll be given a mass of one reactant and asked to determine how much of another is required or can be produced. You can use a molar mass of any compound to convert a mass into moles. Once you have moles of one thing, use the coefficients to determine moles of another, and then use that compounds molar mass to convert moles of that into grams.

So, the basic outlines of any stoichiometry problem will be something like:

grams --> moles --> moles --> grams

Hope this helps..If not, send me a message...

Answer 2

in case you stick to right here steps you may have the skill to remedy any of those sort of issues. a million) balanced equation. 4FeS2 + 15O2 --> 2Fe2O3 + 8SO3 2) convert the plenty into moles moles of FeS2 = 20.0 g / 119.ninety seven g/mol = 0.167 moles moles O2 = sixteen g / 32 g/mol = 0.500 moles 3) Use the mole ratio between FeS2 and O2 to locate the proscribing reagent. The mole ratio is 4 to fifteen. meaning that for each a million mole of FeS2 you utilize you will could desire to apply 15/4 moles of O2 or 3.seventy 5 moles of O2 Now you merely calculated which you have 0.167 moles of FeS2. so which you will choose 0.167 x 3.seventy 5 or 0.626 moles of O2. properly you haven't any longer have been on condition that plenty. you in basic terms have 0.500 moles. so as meaning each and all the O2 would be used up then the reaction stops. That makes O2 the proscribing REAGENT. 4) Now learn the mole ratio of your limting reagent to SO3. that's 15 to eight. OR, for each mole of O2 used up you will in basic terms produce 8/15 of a mole of SO3. so which you have 0.500 moles of O2, so 0.500 x 8/15 = 0.267 moles of SO3 produced. 5) convert that many moles of SO3 to mass. i will anticipate you recognize a thank you to try this.