Given the reaction: 4NH3+5O2--->4NO+6H2O

When 1.20 moles of ammonia reacts, the total number of moles of products formed is: ?

no idea..... thats why i came for help ....

To determine the total number of moles of products formed, we need to calculate the ratio of moles between the reactants and the products.

By looking at the balanced chemical equation:
4NH3 + 5O2 ---> 4NO + 6H2O

We can see that the ratio is 4:4 for ammonia (NH3) and nitric oxide (NO), and 4:6 for ammonia (NH3) and water (H2O).

Given that we have 1.20 moles of ammonia (NH3), we can calculate the moles of nitric oxide (NO) and water (H2O) produced.

For nitric oxide (NO):
1.20 moles NH3 x (4 moles NO / 4 moles NH3) = 1.20 moles NO

For water (H2O):
1.20 moles NH3 x (6 moles H2O / 4 moles NH3) = 1.80 moles H2O

Therefore, when 1.20 moles of ammonia reacts, the total number of moles of products formed is 1.20 moles of nitric oxide (NO) and 1.80 moles of water (H2O).

To determine the total number of moles of products formed in a reaction, we need to use the stoichiometry of the balanced chemical equation.

In the given reaction: 4NH3 + 5O2 ---> 4NO + 6H2O

The coefficients in the balanced equation represent the mole ratios between reactants and products. According to the balanced equation, 4 moles of ammonia (NH3) react to form 4 moles of nitric oxide (NO) and 6 moles of water (H2O).

Given that 1.20 moles of ammonia (NH3) react, we can use the mole ratio to calculate the moles of products formed.

(1.20 moles NH3) x (4 moles NO / 4 moles NH3) = 1.20 moles NO

Similarly,

(1.20 moles NH3) x (6 moles H2O / 4 moles NH3) = 1.80 moles H2O

Therefore, when 1.20 moles of ammonia (NH3) react, the total number of moles of products formed is 1.20 moles of nitric oxide (NO) and 1.80 moles of water (H2O).

ratio

1.2:4::X:10

or in fraction form

1.2/4=x/10
x=10*1.2/4=you do it