type the correct answer in the box. given: cac₂ + n₂ → cacn₂ + c in this chemical reaction, how many grams…

Explanation:

Step1: Calculate molar mass of $CaCN_2$

The molar mass of $Ca$ is approximately $40.08\ g/mol$, $C$ is $12.01\ g/mol$ and $N$ is $14.01\ g/mol$. So molar mass of $CaCN_2$ is $40.08 + 12.01+2\times14.01= 80.11\ g/mol$.

Step2: Calculate moles of $CaCN_2$

Moles of $CaCN_2=\frac{mass}{molar\ mass}=\frac{265\ g}{80.11\ g/mol}\approx 3.31\ mol$.

Step3: Determine mole - ratio from the balanced equation

From the balanced equation $CaC_2 + N_2\rightarrow CaCN_2 + C$, the mole - ratio of $N_2$ to $CaCN_2$ is $1:1$. So moles of $N_2$ required is also $3.31\ mol$.

Step4: Calculate mass of $N_2$

The molar mass of $N_2$ is $2\times14.01 = 28.02\ g/mol$. Mass of $N_2=moles\times molar\ mass=3.31\ mol\times28.02\ g/mol\approx92.7\ g$.

Answer:

$92.7$