In the reaction N2H4 + 2 H2O2 → N2 + 4 H2O, what are the mole ratios of hydrazine (N2H4) to hydrogen peroxide (H2O2) and hydrazine to water (H2O)?

• A. 1:1 for N2H4:H2O2 and 1:2 for N2H4:H2O
• B. 2:1 for N2H4:H2O2 and 4:1 for N2H4:H2O
• C. 2:2 for N2H4:H2O2 and 2:4 for N2H4:H2O
• D. 1:2 for N2H4:H2O2 and 1:4 for N2H4:H2O

Answer: (D)

Verified step by step guidance

1. Identify the balanced chemical equation given: \(\mathrm{N_2H_4 + 2\ H_2O_2 \rightarrow N_2 + 4\ H_2O}\).
2. From the balanced equation, determine the mole ratio of hydrazine (\(\mathrm{N_2H_4}\)) to hydrogen peroxide (\(\mathrm{H_2O_2}\)) by comparing their coefficients: 1 mole of \(\mathrm{N_2H_4}\) reacts with 2 moles of \(\mathrm{H_2O_2}\), so the ratio is \$1:2$.
3. Next, find the mole ratio of hydrazine (\(\mathrm{N_2H_4}\)) to water (\(\mathrm{H_2O}\)) by comparing their coefficients: 1 mole of \(\mathrm{N_2H_4}\) produces 4 moles of \(\mathrm{H_2O}\), so the ratio is \$1:4$.
4. Express these ratios clearly: \(\mathrm{N_2H_4 : H_2O_2 = 1 : 2}\) and \(\mathrm{N_2H_4 : H_2O = 1 : 4}\).
5. Use these mole ratios to understand the stoichiometric relationships in the reaction, which are essential for calculations involving reactant consumption or product formation.