Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH 3 with 17.0 g O 2? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

The mass of nitric oxide is 12.72 grams

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of ammonia = 8.00 g

Molar mass of ammonia = 17 g/mol

Putting values in equation 1, we get:

Given mass of oxygen gas = 17.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

The given chemical reaction follows:

By Stoichiometry of the reaction:

5 moles of oxygen gas reacts with 4 moles of ammonia

So, 0.53 moles of oxygen gas will react with = of ammonia

As, given amount of ammonia is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

5 moles of oxygen gas produces 4 moles of NO

So, 0.53 moles of oxygen gas will produce = of NO

Now, calculating the mass of NO from equation 1, we get:

Molar mass of NO = 30 g/mol

Moles of NO = 0.424 moles

Putting values in equation 1, we get:

Hence, the mass of nitric oxide is 12.72 grams

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml