If 1.00 mol of nitrogen monoxide gas and 1.00 mol of oxy-gen gas react, what is the limiting reactant and how many moles of NO2 are produced from the reaction

Limiting Reactant = NO

Number of moles of NO2 formed = 1

Explanation:

First thing's first, we have to write out the balanced chemical equatin. This is given as;

NO + O2   -->   NO2

Upon balancing we have;

2NO + O2 --> 2NO2

From the stoichiometry of the reaction, we can tell that 2 moles of NO reacts with 1 mole of O2 to form 2 moles of NO2.

If we have 1 mol of Nitrogen monoxide and 1 mol of oxygen, the limiting reactant is NO.

This is because 1 mol of No would require 0.5 mol of O2. So we have an excess of Oxygen while the NO has been used up.

Limiting reactant = NO

since the mole ratio between NO and NO2 is 2:2 it means that 1 mol of NO would also form 1 mol of NO2.

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2