Question

calcium nitride (ca3n2) reacts with water to produce ammonia (nh3). calculate the mass of ammonia formed from 67.0 g of ca3n2. use the references to access important values if needed for this question. 3 item attempts remaining. numeric input field. try another version. submit answer

Explanation:

Step1: Write the balanced chemical equation

$Ca_3N_2 + 6H_2O=3Ca(OH)_2 + 2NH_3$

Step2: Calculate the molar mass of $Ca_3N_2$

The molar mass of $Ca$ is approximately $40.08\ g/mol$ and of $N$ is approximately $14.01\ g/mol$. So, $M_{Ca_3N_2}=3\times40.08 + 2\times14.01=120.24+28.02 = 148.26\ g/mol$

Step3: Calculate the number of moles of $Ca_3N_2$

$n_{Ca_3N_2}=\frac{m_{Ca_3N_2}}{M_{Ca_3N_2}}=\frac{67.0\ g}{148.26\ g/mol}\approx0.452\ mol$

Step4: Determine the mole - ratio between $Ca_3N_2$ and $NH_3$

From the balanced equation, the mole - ratio $n_{Ca_3N_2}:n_{NH_3}=1:2$. So, $n_{NH_3}=2\times n_{Ca_3N_2}=2\times0.452\ mol = 0.904\ mol$

Step5: Calculate the molar mass of $NH_3$

$M_{NH_3}=14.01+3\times1.01=14.01 + 3.03=17.04\ g/mol$

Step6: Calculate the mass of $NH_3$

$m_{NH_3}=n_{NH_3}\times M_{NH_3}=0.904\ mol\times17.04\ g/mol\approx15.4\ g$

Answer:

$15.4$