The mass of 2 moles of H2 gas = 2.00 x 2 = 4.00 g
You must first convert the mass of each reactant into moles of each reactant. Having the same mass does not mean that the amount of each reactant is the same, because each reactant has its own unique molar mass. Refer to the related link below for instructions on determining limiting reactants, also called limiting reagents.
yes it does
The mass of 2 moles of H2 gas = 2.00 x 2 = 4.00 g
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The Limiting Reactant is the reactant that runs out first in a reaction.
You must first convert the mass of each reactant into moles of each reactant. Having the same mass does not mean that the amount of each reactant is the same, because each reactant has its own unique molar mass. Refer to the related link below for instructions on determining limiting reactants, also called limiting reagents.
When calculating the theoretical yield of a product within a reaction, the idea is to convert mass reactant --> mass product; in other words, "how many grams of product X will N grams reactant A and N grams reactant B yield (create)?" Whichever mass is the lowest is considered the theoretical yield (in other words, the reactant that produces the least amount of product).__A + __B --> __Xmass reactant A => mass product X (mass A: mass X)mass reactant B => mass product X (mass B: mass X)In order to calculate the theoretical yield, you need to convert the mass of reactant A to the mass of product X AND the mass of reactant B to the mass of product X.1. Multiply the mass of the reactant by the number of molecules (or moles) X and by the molar mass of X.2. Divide the above by the molar mass of reactant (which is multiplied by the number of molecules [or moles] of reactant).Do this for each reactant involved.- FormulaMass reactant * # molecules (moles) product X1 * molar mass product X--------- # molecules (moles) reactant * molar mass reactant= Mass Product X- Conversion FactorMass reactant * 1 mol reactant * # molecules product X * molar mass product X-------------- molar mass reactant - # molecules reactant --- 1 mol product X= Mass Product X1the # molecules is obtained from the balanced equation. For clarification, I stated # molecules in place of mol; however, on practice problems and in textbook tutorials on how to solve problems in regards to stoichiometry, it is likely it will say mol or moles instead of # molecules.Ex. Ca(NO3)2 + 2NaF --> CaF2 + 2NaNO3What is the theoretical yield of CaF2 (product X) when 43.5g Ca(NO3)2 (reactant A) react with 39.5g NaF (reactant B)?43.5g Ca(NO3)2 * 1 mol Ca(NO3)2 * 1 molecule1 CaF2 * 78.08g CaF2-------------- 164.1g Ca(NO3)2 ----- 1 molecule1 Ca(NO3)2 - 1 mol NaF= 22.3g CaF236.5g NaF * 1 mol NaF * 1 molecule1 CaF2 * 78.08g CaF2------------ 41.99g NaF --- 2 molecules1 NaF --- 1 mol CaF2= 36.7g CaF2The theoretical yield of CaF2 is 22.3g, as it is the lowest amount of product created. In this case, the limiting reagent (the reactant that produced the least product) is Ca(NO3)2 and the reagent in excess is NaF."A chain is only as strong as its weakest link".
yes it does
Balanced chemical equation along with the stoichiometric ratios derived from that chemical reaction. A + B --> 2C mass of A * 1/molar mass of A = moles of A Moles of A * 2 moles of C/mole of A = moles of C Moles of C * molar mass of C = mass of C Also, you must think about limiting reagents, because if there is not enought reactant B to react with the amount of reactant A then the amount of reactant B will limit the production of product C!
The dog named Fluffly is equal to the mass of the reactant
This is the law of mass conservation.
The mass of 2 moles of H2 gas = 2.00 x 2 = 4.00 g
The amount of matter involved in a chemical reaction does not change. The total mass of the reactant must equal the total mass of the products.
The Limiting Reactant is the smaller number once you compare the two reactants with one product. The product that you are comparing them both with must be the same. The Excess Reactant is the larger number, or the amount left over in the chemical reaction.
It is possible to have ten grams of anything. Specifying the total weight tells you nothing about which reactant you have or what reaction it will undergo.
It is not mandatory.
Law of Conservation of Mass. The the number of the compound or elements in the reactant is equal to the product.