Question

Fertilizer The compound calcium cyanamide (CaNCN) is used as a nitrogen source for crops. To obtain this compound, calcium carbide is reacted with nitrogen at high temperatures. $$ \mathrm{CaC}_{2}(\mathrm{s})+\mathrm{N}_{2}(\mathrm{g}) \rightarrow \mathrm{CaNCN}(\mathrm{s})+\mathrm{C}(\mathrm{s}) $$ What mass of CaNCN can be produced if 7.50 $\mathrm{mol}$ of $\mathrm{CaC}_{2}$ reacts with 5.00 $\mathrm{mof} \mathrm{N}_{2} ?$

          Fertilizer The compound calcium cyanamide (CaNCN) is used as a nitrogen source for crops. To
obtain this compound, calcium carbide is reacted with nitrogen at high temperatures.
$$
\mathrm{CaC}_{2}(\mathrm{s})+\mathrm{N}_{2}(\mathrm{g}) \rightarrow \mathrm{CaNCN}(\mathrm{s})+\mathrm{C}(\mathrm{s})
$$
What mass of CaNCN can be produced if 7.50 $\mathrm{mol}$ of $\mathrm{CaC}_{2}$ reacts with 5.00 $\mathrm{mof} \mathrm{N}_{2} ?$

Added by Robin P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Preeti Kumari

01/26/2022

Step 1

The molar mass of CaNCN is: $$40 (Ca) + 14 (N) + 12 (C) = 66 \, \text{g/mol}$$ Show more…

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Fertilizer The compound calcium cyanamide (CaNCN) is used as a nitrogen source for crops. To obtain this compound, calcium carbide is reacted with nitrogen at high temperatures. $$ mathrm{CaC}_{2}(mathrm{s})+mathrm{N}_{2}(mathrm{g}) ightarrow mathrm{CaNCN}(mathrm{s})+mathrm{C}(mathrm{s}) $$ What mass of CaNCN can be produced if 7.50 $mathrm{mol}$ of $mathrm{CaC}_{2}$ reacts with 5.00 $mathrm{mol}$ of $mathrm{N}_{2} ?$