Final answer:
To convert 175 kg of methane into HCN, we need to determine the masses of ammonia and molecular oxygen required for this synthesis. The number of moles of ammonia required is 2 times the number of moles of methane, and the number of moles of molecular oxygen required is equal to the number of moles of methane. Multiplying these moles by their respective molar masses gives us the mass of ammonia and molecular oxygen required.
Step-by-step explanation:
To convert 175 kg of methane into HCN, we need to determine the masses of ammonia and molecular oxygen required for this synthesis. Firstly, let's calculate the number of moles of methane using its molar mass. The molar mass of methane (CH4) is 16.04 g/mol. Since the given mass is 175 kg (175,000 g), we can divide it by the molar mass to get the number of moles: 175,000 g / 16.04 g/mol = 10906.86 mol.
According to the balanced chemical equation for the synthesis of HCN, 1 mole of methane reacts with 2 moles of ammonia (NH3) and 1 mole of molecular oxygen (O2). So, the number of moles of ammonia required is 2 times the number of moles of methane (2 * 10906.86 mol), and the number of moles of molecular oxygen required is equal to the number of moles of methane (10906.86 mol).
To calculate the masses of ammonia and molecular oxygen required, we multiply the number of moles by their respective molar masses. The molar mass of ammonia (NH3) is 17.03 g/mol, so the mass of ammonia required is (2 * 10906.86 mol) * 17.03 g/mol = 370312.46 g. The molar mass of molecular oxygen (O2) is 32.00 g/mol, so the mass of molecular oxygen required is 10906.86 mol * 32.00 g/mol = 348971.52 g.