For the reaction between nitrogen and oxygen to form nitric oxide, beginning with 0.067 mol of N2,
N2(g) + O2(g)= 2 NO(g)
a. how many moles of O2 are required to completely consume the N2?
b. how many moles of NO are obtained when the N2 is completely reacted?
You can convert from anything to anything by using the coefficient in the balanced equation.
a. 0.067 mol N2 x (1 mol O2/1 mol N2) = ?
b. 0.067 mol N2 x (2 mol NO/1 mol N2) = ?
Note that the unit you don't want to keep cancels but the unit to which you wish to convert stays.
Yes.
To find the answers to these questions, you can use the stoichiometry of the reaction. Stoichiometry is the relationship between the amounts of reactants and products in a chemical reaction.
a. To determine how many moles of O2 are required to completely consume the N2, you can use the stoichiometric ratio between N2 and O2 in the balanced equation. According to the balanced equation, for every 1 mole of N2, 1 mole of O2 is needed.
Given that you have 0.067 moles of N2, you can set up a simple ratio:
0.067 moles of N2 : x moles of O2
Using the stoichiometric ratio of 1:1, you can determine that x moles of O2 is also equal to 0.067 moles.
Therefore, you would need 0.067 moles of O2 to completely consume the N2.
b. To find the number of moles of NO obtained when the N2 is completely reacted, you can again use the stoichiometric ratio from the balanced equation. According to the balanced equation, for every 1 mole of N2, 2 moles of NO are produced.
Using the same amount of 0.067 moles of N2, you can set up the following ratio:
0.067 moles of N2 : x moles of NO
Using the stoichiometric ratio of 1:2, you can determine that x moles of NO is equal to 0.067 moles multiplied by 2:
x = 0.067 moles * 2 = 0.134 moles
Therefore, you would obtain 0.134 moles of NO when the N2 is completely reacted.
So the answers would be
a. 0.067
b. 0.134