Answer is: 92.638 g grams of nitrogen must be consumed.
Balanced chemical reaction: CaC₂ + N₂ → CaCN₂ + C.
m(CaCN₂) = 265 g; mass of calcium cyanamide.
M(CaCN₂) = 80.1 g/mol; molar mass of calcium cyanamide.
n(CaCN₂) = 265 g ÷ 80.1 g/mol.
n(CaCN₂) = 3.31 mol; amount of calcium cyanamide.
From balanced chemical reaction: n(CaCN₂) : n(N₂) = 1 : 1.
n(N₂) = 3.31 mol; amount of nitrogen.
m(N₂) = n(N₂) · M(N₂).
m(N₂) = 3.31 mol · 28 g/mol.
m(N₂) = 92.638 g; mass of nitrogen.
92.638 grams of nitrogen gas must be consumed to produce 265 grams of calcium cyanide.
Grams or mass of any substance will be calculated from moles as:
n = W/M, where
W = required mass
M = molar mass
Given chemical reaction is:
Calcium carbide + N₂ → Calcium cyanide + C
Moles of formed calcium cyanide = 265g / 80.1 g/mol = 3.31 mol
From the stoichiometry of the reaction, it is clear that:
1 mole of N₂ consumed = to produce 1 mole of calcium cyanide
To produce 3.31 mole of calcium cyanide = 3.31 moles of N₂ will consumed
Now we calculate the mass of N₂ from their moles as:
W = n × M
W = 3.31 ×28 = 92.638 g
Hence, reaction requires 92.638 g of N₂.
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https://brainly.com/question/1034638
