Homework Help: Chem

Posted by Anonymous on Tuesday, April 20, 2010 at 1:41pm.

Hi! I need help with this problem, also I was wondering what kind of problem is this... limiting reactant?calculate the mass of hydrogen cyanide that could be produced by the complete reaction of 500.0 g of ammonia, 700.0 g of oxygen and 400.0 g of methane according to the equation below, assumming 80.0% efficiency of the reaction.

2NH3(g)+3O2(g)-->2HCN(g)+6H2O(g)

Chem - DrBob222, Tuesday, April 20, 2010 at 5:32pm
Yes, it's a limiting reagent problem.
You must convert each reactant to moles. moles = grams/molar mass.

Using the coefficients in the balanced equation, convert each of the reactant moles to moles of a product, say HCN. The smallest value of HCN moles will the correct value and the reactant producing that will be the limiting reagent. Convert that (moles) to grams, then multiply by 0.80 to find the actual amount produced.

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