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 $CaCN_2$

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

Step2: Calculate moles of $CaCN_2$

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

Step3: Determine mole ratio

From 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 $N_2$

The molar - mass of $N_2$ is $M_{N_2}=2\times14.01 = 28.02\ g/mol$. The mass of $N_2$, $m_{N_2}=n_{N_2}\times M_{N_2}=3.31\ mol\times28.02\ g/mol\approx92.7\ g$

Answer:

$92.7$