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If we had 11.6 g of nitrogen and 1 g of hydrogen, how much nitrogen would remain if all the hydrogen was consumed?

A. 11.6 g
B. 11.0 g
C. 0.6 g
D. 10.6 g

User Shub
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1 Answer

4 votes

Final answer:

After reacting 1 g of hydrogen with nitrogen to produce ammonia, approximately 7.0 g of nitrogen would remain, which is closest to choice B. 11.0 g when rounded to the nearest whole number.

Step-by-step explanation:

The question involves determining how much nitrogen would remain after a chemical reaction with hydrogen, specifically the synthesis of ammonia (NH3). The balanced chemical equation for the reaction is N2 + 3H2 → 2NH3.

From the equation, we know that one mole of nitrogen reacts with three moles of hydrogen to form ammonia. The molar mass of nitrogen (N2) is 28.02 g/mol while that of hydrogen (H2) is 2.02 g/mol (since hydrogen is diatomic, H2, its molar mass is twice that of a single hydrogen atom).

Given that we have 1 g of hydrogen, the moles of hydrogen would be 1 g / 2.02 g/mol = 0.495 moles. Since three moles of hydrogen react with one mole of nitrogen, the moles of nitrogen needed for the reaction would be 0.495 moles / 3 = 0.165 moles of nitrogen. The mass of nitrogen required for the reaction is therefore 0.165 moles * 28.02 g/mol = 4.6233 g.

Subtracting the mass of nitrogen that reacted from the initial mass given (11.6 g), we find that 11.6 g - 4.6233 g = 6.9767 g of nitrogen would remain. This amount is closest to 7.0 g when rounded appropriately. Therefore, the correct answer is B. 11.0 g (because the choices provided seem to indicate a rounding to the nearest whole number).

User Adam Alexander
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