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50g Nitrogen and 10g Hydrogen forms Ammonia.
1. Which is the Limiting Reagent?
2. Calculate no. of moles of Ammonia formed.
3. Calculate number of moles of Nitrogen used to form the calculated Ammonia.
50g Nitrogen and 10g Hydrogen forms Ammonia.
1. Which is the Limiting Reagent?
2. Calculate no. of moles of Ammonia formed.
3. Calculate number of moles of Nitrogen used to form the calculated Ammonia.
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Answer:
Let us write the balanced equation
N2 + 3H2 → 2NH3
Now calculate the number of moles
Number of moles of N2 = 50 kg of N2 = 50 X 10 3 g/1 kg x 28g = 17.86 x 10 2 mole
Number of moles of H2 = 10 kg of N2 = 10 X 103 g/ 1 kg x 2 = 4.96X 103 mol
According to the above equation 1 mole of N2 reacts with 3 moles H2.
That is 17.86 x 10 2 mole of N2 reacts with ------moles of H2
= 3/1 X 17.86 x 10 2 = 5.36 x 103 moles.
Here we have 4.96X 103 mol of hydrogen. Hence Hydrogen is the limiting reagent.
Let us calculate the amount ammonia formed by reacting 4.96X103 moles Hydrogen
3 moles of hydrogen -------2 moles of NH3
4.96 x103 moles Hydrogen -----?
= 4.96 x103 X ⅔
= 3.30 x 103 moles of NH3
Let us write the balanced equation
N2 + 3H2 → 2NH3
Now calculate the number of moles
Number of moles of N2 = 50 kg of N2 = 50 X 10 3 g/1 kg x 28g = 17.86 x 10 2 mole
Number of moles of H2 = 10 kg of N2 = 10 X 103 g/ 1 kg x 2 = 4.96X 103 mol
According to the above equation 1 mole of N2 reacts with 3 moles H2.
That is 17.86 x 10 2 mole of N2 reacts with ------moles of H2
= 3/1 X 17.86 x 10 2 = 5.36 x 103 moles.
Here we have 4.96X 103 mol of hydrogen. Hence Hydrogen is the limiting reagent.
Let us calculate the amount ammonia formed by reacting 4.96X103 moles Hydrogen
3 moles of hydrogen -------2 moles of NH3
4.96 x103 moles Hydrogen -----?
= 4.96 x103 X ⅔
= 3.30 x 103 moles of NH3