If 3.670 g of nitrogen combines with 0.5275 g of hydrogen to yield compound X, how many grams of nitrogen would combine with 1.575 g of hydrogen to make the same compound? Is X ammonia (NH3) or hydrazine (N2H4)?

Verified step by step guidance

1. Step 1: Determine the ratio of nitrogen to hydrogen in the original compound by dividing the mass of nitrogen by the mass of hydrogen: \( \frac{3.670 \, \text{g N}}{0.5275 \, \text{g H}} \).
2. Step 2: Use the ratio from Step 1 to find out how many grams of nitrogen would combine with 1.575 g of hydrogen. Set up a proportion: \( \frac{3.670 \, \text{g N}}{0.5275 \, \text{g H}} = \frac{x \, \text{g N}}{1.575 \, \text{g H}} \) and solve for \( x \).
3. Step 3: Calculate the molar mass of ammonia (NH3) and hydrazine (N2H4) to compare with the ratio obtained. Ammonia has a molar mass of approximately 17.03 g/mol, and hydrazine has a molar mass of approximately 32.05 g/mol.
4. Step 4: Determine the nitrogen to hydrogen ratio in ammonia and hydrazine. For ammonia, the ratio is \( \frac{14.01 \, \text{g N}}{3.02 \, \text{g H}} \), and for hydrazine, it is \( \frac{28.02 \, \text{g N}}{4.04 \, \text{g H}} \).
5. Step 5: Compare the calculated nitrogen to hydrogen ratio from Step 2 with the ratios for ammonia and hydrazine to determine which compound matches the experimental data.