1. **State the problem:** Calculate the mass of HCN produced when 8.43 grams of N₂ react. 2. **Write the balanced chemical equation:** The reaction is typically $ N_2 + 3H_2 \rightarrow 2NH_3 $, but since HCN is involved, assume the reaction producing HCN from N₂ is balanced as: $$ N_2 + 3CH_4 \rightarrow 2HCN + 6H_2 $$ (If the exact reaction is different, the molar ratio of N₂ to HCN is 1:2.) 3. **Calculate molar masses:** - Molar mass of $ N_2 $ is given as 28.02 g/mol. - Molar mass of HCN is calculated as: $$ 1.008 + 12.011 + 19.007 = 32.026 \text{ g/mol} $$ 4. **Convert given mass of N₂ to moles:** $$ \text{moles of } N_2 = \frac{8.43}{28.02} \approx 0.301 \text{ mol} $$ 5. **Use mole ratio to find moles of HCN produced:** $$ 0.301 \text{ mol } N_2 \times \frac{2 \text{ mol } HCN}{1 \text{ mol } N_2} = 0.602 \text{ mol } HCN $$ 6. **Calculate mass of HCN produced:** $$ \text{mass of } HCN = 0.602 \times 32.026 = 19.27 \text{ g} $$ **Final answer:** $$ \boxed{19.27 \text{ grams of HCN}} $$