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How many grams of hydrogen are necessary to react completely with 2.3 moles of nitrogen, in the reaction N2+3H2 = 2NH3?

Answer 1

Cameron Andrews

4.6 g

Here's how we can set it up,

#"mass of hydrogen"="2.3 mols " N_2*("3 mols "H_2)/("1 mol "N_2)*((2*1)"g/mol")/("3 mols "H_2)=4.6 g#

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Answer 2

Kai Bowman

To find out how many grams of hydrogen are needed to react completely with 2.3 moles of nitrogen in the given reaction ( N_2 + 3H_2 \rightarrow 2NH_3 ), we can use the stoichiometry of the reaction. According to the balanced equation, 3 moles of hydrogen react with 1 mole of nitrogen. So, to find out how many grams of hydrogen are needed for 2.3 moles of nitrogen:

[ \text{Moles of } H_2 = 3 \times \text{moles of } N_2 ] [ \text{Moles of } H_2 = 3 \times 2.3 ] [ \text{Moles of } H_2 = 6.9 ]

Now, to convert moles of ( H_2 ) to grams:

[ \text{Grams of } H_2 = \text{moles of } H_2 \times \text{molar mass of } H_2 ] [ \text{Grams of } H_2 = 6.9 \times 2.02 ] [ \text{Grams of } H_2 = 13.938 ]

Rounded to three significant figures, the answer is 13.9 grams of hydrogen.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.