Question

2 na₃n → 6 na + n₂

1. given 0.98 moles of n₂, how many moles of na₃n are required?

1. given 1.25 moles of na₃n, how many moles of na are produced?

2 al + 3 s → al₂s₃

1. if 3.12 moles of al₂s₃ are created, how many moles of s are also used?

1. if 0.32 moles of s are used, how many moles of al are used?

Explanation:

Step1: Analyze the stoichiometry of the reaction

For the reaction \(2\text{Na}_3\text{N}
ightarrow6\text{Na}+\text{N}_2\), the mole ratio of \(\text{Na}_3\text{N}\) to \(\text{N}_2\) is \(2:1\).

Step2: Calculate the moles of \(\text{Na}_3\text{N}\)

If \(n(\text{N}_2) = 0.98\space mol\), using the mole ratio \(\frac{n(\text{Na}_3\text{N})}{n(\text{N}_2)}=\frac{2}{1}\), then \(n(\text{Na}_3\text{N})=2\times n(\text{N}_2)\).
Substitute \(n(\text{N}_2) = 0.98\space mol\) into the formula: \(n(\text{Na}_3\text{N})=2\times0.98 = 1.96\space mol\).

Step3: Analyze the second reaction for question 10

For the reaction \(2\text{Na}_3\text{N}
ightarrow6\text{Na}+\text{N}_2\), the mole ratio of \(\text{Na}_3\text{N}\) to \(\text{Na}\) is \(2:6 = 1:3\).

Step4: Calculate the moles of \(\text{Na}\)

If \(n(\text{Na}_3\text{N})=1.25\space mol\), using the mole ratio \(\frac{n(\text{Na})}{n(\text{Na}_3\text{N})}=\frac{3}{1}\), then \(n(\text{Na}) = 3\times n(\text{Na}_3\text{N})\).
Substitute \(n(\text{Na}_3\text{N})=1.25\space mol\) into the formula: \(n(\text{Na})=3\times1.25=3.75\space mol\).

Step5: Analyze the reaction \(2\text{Al}+3\text{S}

ightarrow\text{Al}_2\text{S}_3\) for question 11
The mole ratio of \(\text{S}\) to \(\text{Al}_2\text{S}_3\) is \(3:1\).

Step6: Calculate the moles of \(\text{S}\)

If \(n(\text{Al}_2\text{S}_3)=3.12\space mol\), using the mole ratio \(\frac{n(\text{S})}{n(\text{Al}_2\text{S}_3)}=\frac{3}{1}\), then \(n(\text{S})=3\times n(\text{Al}_2\text{S}_3)\).
Substitute \(n(\text{Al}_2\text{S}_3)=3.12\space mol\) into the formula: \(n(\text{S})=3\times3.12 = 9.36\space mol\).

Step7: Analyze the reaction for question 12

The mole ratio of \(\text{Al}\) to \(\text{S}\) is \(2:3\).

Step8: Calculate the moles of \(\text{Al}\)

If \(n(\text{S}) = 0.32\space mol\), using the mole ratio \(\frac{n(\text{Al})}{n(\text{S})}=\frac{2}{3}\), then \(n(\text{Al})=\frac{2}{3}\times n(\text{S})\).
Substitute \(n(\text{S}) = 0.32\space mol\) into the formula: \(n(\text{Al})=\frac{2\times0.32}{3}\approx0.21\space mol\).

Answer:

1. \(1.96\space mol\)
2. \(3.75\space mol\)
3. \(9.36\space mol\)
4. \(0.21\space mol\)