mols A = 1. How many moles of C will that form? Using the coefficients in the balanced equation, convert moles A to moles C. 1 mole A x (3 moles C/1 mole A) = 3 moles C.
moles B = 1. How many moles of C will that form? Same process as above, convert moles B to moles C. 1 mole B x (3 moles C/2 moles B) = 3/2 = 1.5 moles C.
3 moles C and 1.5 moles C don't agree and one of those answers must be wrong. The correct answer in limiting reagent problems is ALWAYS the smaller one and the reagent producing that value is the limiting reagent. So 1.5 moles C is the theoretical yield and B is the limiting reagent. (The question doesn't ask but we can calculate how much A isused up and how much is un-reacted). That will be 1 mole B x (1 mole A/2 moles B) = 1/2 or 0.5 mole A used; therefore, there is 0.5 mole A remaining un-reacted.)
Suppose 3.50g each of sulfamic acid and sodium nitrite were allowed to react together. What would be the theoretical yield, in moles, of N2. Equation: NaNO2 + NH3SO3 -> N2 + H2O + NaHSO4 Notes: The theoretical yield of N2 can be
How are these values used to determine percent? actual yield is quantity of a product found to be formed in a chemical reaction and theoretical yield is the amount of product predicted theoretical yield is larger because in
how do you calculate theoretical yield of something? I don't know where to find the formula You go to the balanced chemical equation, and look at the mole ratio between the reactants and products. The theoretical yield is the
Write the overall reaction equation for the synthesis of aluminum potassium sulphate dodecahydrate, then determine the theoretical yield. 2Al+2KOH+4H2SO4+22H2O --> 2KAl(SO4)2*12H20 I don't know how to calculate theoretical yield
I have this question and I am pretty sure on what to use to solve it but I am just stuck. The reaction of 8 g of hydrogen and 28 g of carbon monoxide gave 16 g of methanol. What was the theoretical yield if the percent yield was
how do you distinquish between a limiting reactant and the excess reactant in a chemical reaction? b) how do you distinguish between the theoretical yield and actual yield in stoichiometric calculations and how does the value of
we're given the equation: C6H6(l)+Br2(l) --> C6H5Br(l)+HBr(g) you need to prepare 50.0g pf bromobenzene and you expect no more than a 75% yield. How much benzene should you begin with if the yield is 75%. i know that % yield =
Fe can be prepared as 2 Al + Fe2O3 ----> 2 Fe + Al2O3. Suppose that 0.450 moles of Fe2O3 are reacted with an excess of Al. Suppose that 43.6 grams of Fe are obtained. What is the percent yield of Fe? a) 16.2% b) 60.7% c) 86.7% d)
In the Reaction CO+2H²-->CH³OH, 1.27 g of CH³OH are made in the lab. The Percent yield of this reaction is___. Would the answer be 42? Pick a number, any number. You need to know how much CO OR H2 you started with. As it