Question
Al2O3(s)+6NO(g)---->5N2(g)+6H2O(l)
how many grams of Nitric Oxide are required to produce 145g of nitrogen in the following reaction?
how many grams of Nitric Oxide are required to produce 145g of nitrogen in the following reaction?
Answers
Steve
as written, 6 moles of NO produce 5 moles of N2
(The equation doesn't balance, but I assume there are other products involved - ?)
mass of N2 = 28
145g NO = 145/28 = 5.18 moles
5.18mN2 * 6mNO/5mN2 = 6.21mNO
mass of NO = 30
6.21m * 30g/m = 186g
(The equation doesn't balance, but I assume there are other products involved - ?)
mass of N2 = 28
145g NO = 145/28 = 5.18 moles
5.18mN2 * 6mNO/5mN2 = 6.21mNO
mass of NO = 30
6.21m * 30g/m = 186g