Question

25g of NH3 is mixed with 4 moles of O2 in given reaction.
4NH3(g)+5O2(g)-->4NO(g)+6H2O(1)
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what mass of NO is formed?
What mass of H2O is formed?

Answer 1

First we determine the limiting reactant.

The molar mass of NH3 is 17 g/mol.
Getting the moles of NH3, we just divide the given mass by the molar mass:
25 g / 17 g/mol = 1.47 mol NH3

We determine the moles of NO produced by making mole ratios from the balanced reaction, such as:
4 mol NO / 4 mol NH3 , and
4 mol NO / 5 mol O2

We multiply the moles of O2 and NH3 by the corresponding mole ratio to get the moles of NO. the one who produces the smaller number of moles of NO is the limiting reactant:
1.47 mol NH3 * (4 mol NO / 4 mol NH3) = 1.47 mol NO
4 mol O2 * (4 mol NO / 5 mol O2) = 3.2 mol NO

Therefore, NH3 is limiting.
Now that we know the moles of NO produced from 1.47 mol NH3, we multiply this value to the molar mass to get the mass. Molar mass of NO is 30 g/mol:
1.47 mol NO * 30 g NO / mol NO = 44.1 g NO

For the second question mass of H2O formed), use the same method. Hope this helps~ `u`

Answer 2

27.5

Answer 3

What MassH2Ois?

Answer 4

So,saport it

Answer 5

what mass of no is formed

Answer 6

take

Answer 7

solve it