Question

1. carbon disulfide (cs2) reacts with oxygen to form carbon dioxide and sulfur dioxide. if we have 60.0 g oxygen, what is the maximum amount of sulfur dioxide that we can obtain?

Explanation:

Step1: Write the balanced chemical equation

$CS_2 + 3O_2
ightarrow CO_2+2SO_2$

Step2: Calculate the molar mass of $O_2$

The molar mass of $O_2$ is $M_{O_2}=2\times16 = 32$ g/mol. The number of moles of $O_2$, $n_{O_2}=\frac{m}{M}=\frac{60.0}{32}= 1.875$ mol.

Step3: Determine the mole - ratio between $O_2$ and $SO_2$

From the balanced equation, the mole - ratio of $O_2$ to $SO_2$ is $3:2$.

Step4: Calculate the number of moles of $SO_2$

Let the number of moles of $SO_2$ be $n_{SO_2}$. Using the mole - ratio, $n_{SO_2}=\frac{2}{3}n_{O_2}=\frac{2}{3}\times1.875 = 1.25$ mol.

Step5: Calculate the molar mass of $SO_2$

The molar mass of $SO_2$ is $M_{SO_2}=32 + 2\times16=64$ g/mol.

Step6: Calculate the mass of $SO_2$

The mass of $SO_2$, $m_{SO_2}=n_{SO_2}\times M_{SO_2}=1.25\times64 = 80$ g.

Answer:

80 g