In the following reaction, how many grams of ammonia (NH3) will produce 300 grams of N2? 4NH3 + 6NO d 5N2 + 6H2O
Follow the steps.
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To determine the grams of ammonia (NH3) required to produce 300 grams of N2, you need to use stoichiometry.
1. Start by examining the balanced chemical equation:
4NH3 + 6NO -> 5N2 + 6H2O
2. Identify the molar mass of NH3. The molar mass of NH3 is approximately 17.03 grams/mol.
3. Find the molar ratio between NH3 and N2 from the balanced chemical equation. In this case, the ratio is 4 moles of NH3 to 5 moles of N2.
4. Calculate the moles of N2. Since 300 grams of N2 were given, divide this value by the molar mass of N2. The molar mass of N2 is approximately 28.02 grams/mol. So, 300 grams of N2 would be equal to 10.71 moles (300 g / 28.02 g/mol).
5. Use the molar ratio to find the moles of NH3. Multiply the moles of N2 by the molar ratio of NH3 to N2, which is 4/5. Therefore, the moles of NH3 would be (10.71 moles of N2) x (4 moles of NH3 / 5 moles of N2) = 8.568 moles of NH3.
6. Finally, convert the moles of NH3 into grams. Multiply the moles of NH3 by the molar mass of NH3, which is approximately 17.03 grams/mol. Thus, the grams of NH3 required to produce 300 grams of N2 would be (8.568 moles of NH3) x (17.03 g/mol) = 146 grams of NH3.
Therefore, 146 grams of ammonia (NH3) are required to produce 300 grams of N2.