Consider the reaction 4 HCl + O2 → 2 H2O + 2 Cl2. How many moles of Cl2 can be produced if 62.4 g of HCl reacts?

When 24.5g of NH 3 reacts, the actual yield of H 2O is 26.5g.  What is the percent yield? 4NH 3( g) + 6NO( g) → 5N 2( g) + 6H 2O( l)

Calculate the quantity of O2 would be required to generate 13.0 mol of NO2 in the reaction below assuming the reaction has only 66.5% yield. 2 NO (g) + O2 (g)→2 NO2 (g)

What mass of HCl will be produced when 24.9 g of AlCl₃ are reacted according to this chemical equation? 2 AlCl₃ + 3 H₂O → Al₂O₃ + 6 HCl

When 85.0 g of CH 4 are mixed with 160. g of O 2 what is the maximum amount of CO 2 that can be produced?CH 4  + 2O 2  → CO 2  + 2H 2O     5.00 moles     2.50 moles     7.81 moles     5.31 moles

Given that the reaction below has a yield of 84.36%, If you needed to create 26.29 g of SbCl3 Determine  the theoretical yield of SbCl3 in grams . 2 Sb + 3 Cl2 → 2 SbCl3

How many grams of NO are required to produce 145 g of N₂ in the following reaction? 4NH3 + 6NO → 5N2 + 6H₂O O 125 g 186 g O 145 g O 155 g

Iron(III) oxide reacts with carbon monoxide according to the equation:Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)A reaction mixture initially contains 22.35 g Fe2O3Fe2O3 and 15.54 g CO Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

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How many grams of NO will be produced from 55.7 g of NO₂ reacted with excess water in the following chemical reaction? 3 NO₂(g) + H₂O(l) → 2 HNO₃(g) + NO(g)