Question

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. CaC2(s) + N2(g) CaNCN(s) + C(s) What mass of CaNCN can be produced if 7.45 mol CaC2 reacts with 5.85 mol N2?

Answer 1

To find the mass of CaNCN produced, we need to determine the limiting reactant (N2) and use stoichiometry. The expected moles of CaNCN are 5.85 mol, which can be converted to mass using its molar mass.

Step-by-step explanation:

To find the mass of CaNCN produced, we need to determine the limiting reactant and use stoichiometry.

First, we need to find the molar ratio between CaC2 and CaNCN, which is 1:1.

Then, we compare the given number of moles of CaC2 (7.45 mol) and N2 (5.85 mol).

The limiting reactant is the one that produces fewer moles of the desired compound, and in this case, it is N2.

Therefore, N2 limits the amount of CaNCN that can be produced.

Using the molar ratio, we can calculate the moles of CaNCN produced, which is also 5.85 mol.

Finally, we can convert the moles of CaNCN to mass using its molar mass.

1. CaC2 + N2 CaNCN + C
2. Molar ratio: 1:1 between CaC2 and CaNCN
3. Given: 7.45 mol CaC2, 5.85 mol N2
4. Limiting reactant: N2
5. Expected moles of CaNCN: 5.85 mol
6. Calculate mass of CaNCN: moles of CaNCN x molar mass of CaNCN

Answer 2

N2 + CaC2 = CaNCN + C
As you can see, 1 mol of N2 can react completely with 1 mol of CaC2 and 1 mol of CaNCN will be obtained
It means 5 mol of N2 can react completely with 5 mol of CaC2 and 5 mol of CaNCN will be obtained

So, there are 7.5 - 5 = 2.5 odd mole of CaC2 after the reaction
And the mass of obtained CaNCN is
m = n*M = 5*80 = 400g