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The mass of 2 moles of H2 gas = 2.00 x 2 = 4.00 g
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What is the limiting reactant in 2H2 plus O2 equals 2H2O?
There is no limiting reactant in that equation, it's balanced. Four hydrogens on the left, 4 on the right, 2 oxygens on the left, 2 oxygens on the right. If it was 3H2 then it would be oxygen.
Which is the limiting reactant when masses of reactants are same?
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.
Is hydrogen a reactants?
Hydrogen can be a reactant or a product, it depends on the chemical reaction. Anything to the left of the arrow is consumed by the reaction and is thus a reactant, so hydrogen is a reactant in the reaction O2 + 2H2 -> 2H2O. A product is on the right of the arrow and is produced by the reaction, so hydrogen is a product in the reaction Zn + 2HCl -> ZnCl2 + H2
Does the mass of a solid reactant affect the reaction rate?
yes it does
What is the reactant of the mass?
The mass of 2 moles of H2 gas = 2.00 x 2 = 4.00 g
Which reactant is the limiting reagent and why 2H2 O2?
This depends on the proportion of these gases in the reactor.
What is is the principle of conservation of mass?
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.
What is the reactant of 10.0 grams of total mass What is 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.
In a correctly written nuclear equation what is true about the total mass number on the reactant side as compared to the total mass number on the product side?
the total mass number should be equal on both sides. conservation of mass law.
What is the reactant in 2H2O equals 2H2 plus O2?
There is no limiting reactant in that equation, it's balanced. Four hydrogens on the left, 4 on the right, 2 oxygens on the left, 2 oxygens on the right. If it was 3H2 then it would be oxygen.
What is the limiting reactant in 2H2 plus O2 equals 2H2O?
There is no limiting reactant in that equation, it's balanced. Four hydrogens on the left, 4 on the right, 2 oxygens on the left, 2 oxygens on the right. If it was 3H2 then it would be oxygen.
Is 2H2 O2---2H20 balanced?
2H2 + O2 ---> 2H20 is balanced when total numbers of atoms of EACH element seperately are equal on both sides ('Reactant' and 'Product' side): Left (2x H2=) 4 H atoms and (1x2 O=) 2 O atoms Right (2x H2=) 4 H's and (2x1 O=) 2 O's
Which is the limiting reactant when masses of reactants are same?
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.
Is hydrogen a reactants?
Hydrogen can be a reactant or a product, it depends on the chemical reaction. Anything to the left of the arrow is consumed by the reaction and is thus a reactant, so hydrogen is a reactant in the reaction O2 + 2H2 -> 2H2O. A product is on the right of the arrow and is produced by the reaction, so hydrogen is a product in the reaction Zn + 2HCl -> ZnCl2 + H2
How do you calculate theoretical yield?
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".
Does the mass of a solid reactant affect the reaction rate?
yes it does
For the following equation SnO2 plus 2H2 equals Sn plus 2H20 how many grams of Sn is formed if 12.5 grams of the first reactant is used?
9,846 g of tin (Sn)
