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Angelina_Jolie [31]
3 years ago
12

According to the following reaction, how many grams of nitrogen monoxide will be formed upon the complete reaction of 31.0 grams

of oxygen gas with excess ammonia? ammonia (g) + oxygen (g) nitrogen monoxide (g) + water (g)
Chemistry
1 answer:
Mumz [18]3 years ago
8 0

23.227 grams of NO is formed upon the complete reaction of 31.0 grams of oxygen gas with excess ammonia.

Explanation:

The balanced chemical equation is:

4NH3 + 5O2 ⇒ 4NO + 6H20

Number of moles will be calculated.

31 grams of oxygen is given

atomic weight of oxygen gas i.e O2 = 32gm/mole

The molar mass of oxygen gas is 32 grams/mole which is equal to one mole of the molecule.

Number of moles (n) = \frac{mass}{atomic mass of one mole of the substance}

                             n=    \frac{31}{32}

                              n = 0.968 moles of oxygen are given for the reaction to occur.

From the balanced chemical equation it can be seen

5 moles of oxygen yielded 4 moles of NO

So, 0.968 moles of oxygen yield x moles of NO

\frac{4}{5} = \frac{x}{0.968 }

4 × 0.968 =5x

x = 0.774 moles of NO will be formed.

To calculate the mass of NO

mass= atomic mass x number of moles

atomic mass of NO is 30.01 grams/mole

putting the values in the formula:

mass = 30.01 x 0.774

          = 23.227 grams of NO is formed.

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