**During estimation of nitrogen present in an organic compound by Kjeldahl’s method, the ammonia evolved from 0.5 g of the compound in Kjeldahl’s estimation of nitrogen, neutralized 10 mL of 1 M H**_{2}SO_{4}. Find out the percentage of nitrogen in the compound.

I will explain how i solved this, please help me find my mistake

first i calculated the number of moles of H_{2}S0_{4} involved using the given volume and concentration.

it came out to be 10^{-2} moles.

In reaction between ammonia and H_{2}SO_{4}, for every 1 mole of sulphuric acid, there are 2 moles of ammonia reacting with it.

so, the number of moles of ammonia must be 2 x 10^{-2} moles.

ammonia has nitrogen to hydrogen ratio as 1:3.

which means the number of moles of nitrogen atoms is (2 x 10^{-2})/4.

which is 5 x 10^{-3}

1 mole of nitrogen atom would have a mass of 14 grams which means the mass of nitrogen here is 5 x 10^{-3} x 14 grams.

which will be 7 x 10^{-2}

the mass of the organic compound is 0.5 gram.

so, to calculate the percentage of nitrogen i did ((7 x 10^{-2})/0.5) x 100

which comes out to be 14 percent

the answer key says that it is 56 percent

where did i go wrong?