Question

How many grams of nitrogen, N2, would be required to react with 6.25 moles hydrogen, H2?

Answer 1

56.88g N2

Step-by-step explanation:

1 mole of N2 will react to 3 moles of H2

so 6.25 moles of H2 will react to 6.25/3 = 2.03 moles of N2

molar mass of N2 = 2(14.01) = 28.02 g/mol

mass of N2 = 2.03 x 28.02 = 56.88 g

Answer 2

58.38 grams of
`\( N_2 \)`, which is the amount needed to react with 6.25 moles of
`\( H_2 \)`.

To calculate the grams of nitrogen
`\( N_2 \)` needed to react with 6.25 moles of hydrogen
`\( H_2 \)`:

1. Identify the molar ratio from the balanced equation
`\( N_2 + 3H_2 \` to
`2NH_3 \)`, which is
`\( 1:3 \)` for
`\( N_2 \)` to

2. Determine the moles of
`\( N_2 \)` needed using this ratio:
`\( \frac{6.25 \text{ moles } H_2}{3} \) gives the moles of \( N_2 \).`

3. Multiply the moles of
`\( N_2 \)` by the molar mass of
`\( N_2 \)` (approximately
`\( 28.02 \)` g/mol) to convert to grams.

4. The calculation yields 58.38 grams of
`\( N_2 \)`, which is the amount needed to react with 6.25 moles of
`\( H_2 \)`.