Question

type the correct answer in the box. given: cac₂ + n₂ → cacn₂ + c in this chemical reaction, how many grams of n₂ must be consumed to produce 265 grams of cacn₂? express your answer to three significant figures. the reaction requires grams of n₂.

Explanation:

Step1: Calculate molar mass of CaCN₂

The molar mass of CaCN₂: $M_{CaCN_2}=40.08 + 12.01+2\times14.01 = 80.11\ g/mol$.

Step2: Find moles of CaCN₂

The number of moles of CaCN₂, $n_{CaCN_2}=\frac{m_{CaCN_2}}{M_{CaCN_2}}=\frac{265\ g}{80.11\ g/mol}\approx3.31\ mol$.

Step3: Determine mole - ratio from equation

From the balanced chemical equation $CaC_2 + N_2
ightarrow CaCN_2 + C$, the mole - ratio of $N_2$ to $CaCN_2$ is 1:1. So, $n_{N_2}=n_{CaCN_2}=3.31\ mol$.

Step4: Calculate mass of N₂

The molar mass of $N_2$ is $M_{N_2}=2\times14.01 = 28.02\ g/mol$. The mass of $N_2$, $m_{N_2}=n_{N_2}\times M_{N_2}=3.31\ mol\times28.02\ g/mol\approx70.5\ g$.

Answer:

70.5