Respuesta :
Answer:
75.59 grams of N2
Explanation:
To find the grams of N2 required to produce 265 grams of CaCN2, we need to use stoichiometry to relate the masses of CaCN2 and N2 in the balanced chemical equation.
From the balanced chemical equation:
1 mol of CaC2 reacts with 1 mol of N2 to produce 1 mol of CaCN2.
We need to find the molar mass of CaCN2 to convert the grams of CaCN2 to moles:
Molar mass of CaCN2 = atomic mass of Ca + atomic mass of C + 2 * atomic mass of N
= 40.08 g/mol + 12.01 g/mol + 2 * 14.01 g/mol
≈ 98.11 g/mol
Now, we can use stoichiometry to find the moles of N2 required:
1 mol of CaCN2 corresponds to 1 mol of N2.
Moles of CaCN2 = Mass of CaCN2 / Molar mass of CaCN2
= 265 g / 98.11 g/mol
≈ 2.698 moles
Since the stoichiometry is 1:1 between CaCN2 and N2, the moles of N2 required will be the same as the moles of CaCN2.
Moles of N2 required = 2.698 moles
Now, to find the grams of N2 required:
Mass of N2 = Moles of N2 * Molar mass of N2
= 2.698 moles * 28.02 g/mol
≈ 75.59 grams
Therefore, the reaction requires approximately 75.59 grams of N2 to produce 265 grams of CaCN2.
