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- Question #a0043 - Socratic
8 4 * 10^(23)"atoms" Your goal here is to use a conversion factor that can take you from moles of zinc to atoms of zinc The idea is that if you know how many atoms you get in one mole of zinc, you can cause this to calculate how many atoms you'd get in 1 4 moles of zinc Now, one mole of any element is said to contain 6 022 * 10^(23) atoms of that element -> this is known as Avogadro's number
- Question #b9b62 - Socratic
See below In order to solve this problem, you will need to be aware of a number called "Avogadro's number " Avogadro's number, 6 022*10^23, details the number of molecules atoms in 1 mole of substance Keeping this in mind, here is the dimensional analysis setup for this particular question (we are converting from moles "S"_2"O"_3 to molecules of "S"_2"O"_3 (using Avogadro's number) to number
- How do you determine the limiting reagent and what is the . . . - Socratic
Now, the theoretical yield corresponds to the amount of product produced if all the moles of reactants that actually react end up producing moles of product Notice that the reaction produces 1 mole of phosphoric acid, "H"_2"PO"_4, and 5 moles of hydrochloric acid, for 1 mole of phosphorus pentachloride and color(red)(5) moles of water
- How many formula units constitute a mass of - Socratic
The number of particles #N -# or in this case molecules #-# of a substance is given by the equation #N = n L#; where #n# is the number of mole and #L# is Avogrado's constant Also, the definition of #n# is given by the equation #n = frac(m)(M)#; where #m# is the mass and #M# is the molar mass Let's substitute the definition of #n# into the
- What is the mass of three moles of ethane? - Socratic
Chemistry The Mole Concept The Mole 1 Answer anor277 Sep 23, 2016
- Question #fbe82 - Socratic
The mixture is 56 33% "KMnO"_4 and 43 67% "K"_2"Cr"_2"O"_7 The keys to solving this problem are the balanced chemical equations for the three redox reactions that take place Now, I assume that you are supposed to write and balance these equations, but I cannot do that here because that would make for a very long answer I wil lalso skip any explanation as to why the reactions produce what
- Question #9ca2c - Socratic
The first thing to do here is use the molar masses of the two reactants to determine how many moles of each you're mixing 82 color(red)(cancel(color(black)("g"))) * "1 mole Cu" (63 546color(red)(cancel(color(black)("g")))) = "1 29 moles Cu" 25 color(red)(cancel(color(black)("g"))) * "1 mole S"_8 (256 5color(red)(cancel(color(black)("g")))) = "0
- Question #2cabc + Example - Socratic
The number of ions present in a given amount of moles of a compound is calculated using Avogadro's number and the number of ions represented in the formula of its solution Example: If we had one mole of NaOH which is a strong base solid dissolved in 1l water, we would have an aqueous solution of ions The number of particles in one mole of NaOH is 6 022xx10^23 The number of Na^+(aq) ions in
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