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)

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.

Hello! This is a stoichiometry problem. To solve it, we need to determine the limiting reactant, which is the reactant that is completely consumed and determines the amount of product that can be produced.

To find the limiting reactant, we compare the number of moles of each reactant to the stoichiometric coefficients in the balanced equation. The reactant that produces the fewest moles of the desired product is the limiting reactant.

First, we need to convert the given masses of each reactant into moles. To do this, we use the molar mass of each substance.

The molar masses are:
NH3: 17.03 g/mol
O2: 32.00 g/mol
CH4: 16.04 g/mol

Converting to moles:
moles of NH3 = 500.0 g / 17.03 g/mol
moles of O2 = 700.0 g / 32.00 g/mol
moles of CH4 = 400.0 g / 16.04 g/mol

Next, we use the stoichiometric coefficients from the balanced equation to determine the number of moles of HCN produced from each reactant.

Using the coefficients:
moles of HCN from NH3 = 2 * (moles of NH3)
moles of HCN from O2 = (3/2) * (moles of O2)
moles of HCN from CH4 = 2 * (moles of CH4)

Now we compare the moles of HCN produced from each reactant to determine the limiting reactant. The reactant that produces the fewest moles of HCN is the limiting reactant.

Finally, once we determine the limiting reactant, we can calculate the mass of HCN produced using stoichiometry.

To include the efficiency of the reaction, we multiply the moles of HCN produced by the conversion factor of 80% (0.80).

Does this explanation help?