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3.2 g sulphur combines with 3.2 g of oxy...

`3.2 g` sulphur combines with `3.2 g` of oxygen, to from a compound in one set of conditions. In another set of conditions `0.8 g` of sulphur combines with `1.2 g` of oxygen to form another compound. State the law illustrated by these chemical combinations.

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To solve the problem, we need to analyze the two sets of combinations of sulfur and oxygen and identify the law that governs these combinations. ### Step-by-Step Solution: 1. **Identify the Masses of Sulfur and Oxygen in the First Combination:** - In the first case, we have: - Mass of sulfur (S) = 3.2 g - Mass of oxygen (O) = 3.2 g 2. **Calculate the Ratio of Sulfur to Oxygen in the First Combination:** - To find the ratio of sulfur to oxygen: \[ \text{Ratio} = \frac{\text{Mass of S}}{\text{Mass of O}} = \frac{3.2 \, \text{g}}{3.2 \, \text{g}} = 1:1 \] 3. **Identify the Masses of Sulfur and Oxygen in the Second Combination:** - In the second case, we have: - Mass of sulfur (S) = 0.8 g - Mass of oxygen (O) = 1.2 g 4. **Calculate the Ratio of Sulfur to Oxygen in the Second Combination:** - To find the ratio of sulfur to oxygen: \[ \text{Ratio} = \frac{\text{Mass of S}}{\text{Mass of O}} = \frac{0.8 \, \text{g}}{1.2 \, \text{g}} = \frac{2}{3} \] 5. **Convert the Ratios to a Common Basis:** - For comparison, we can express both ratios in terms of 1 g of sulfur: - From the first combination: 1 g of S combines with 1 g of O. - From the second combination: 1 g of S combines with \( \frac{1.2 \, \text{g}}{0.8 \, \text{g}} = 1.5 \, \text{g of O} \). 6. **Establish the Ratio of Oxygen in Both Cases:** - The ratios of oxygen combining with 1 g of sulfur are: - First case: 1 g of O - Second case: 1.5 g of O - This can be expressed as: \[ \text{Ratio of O in both cases} = 1:1.5 \text{ or } 2:3 \] 7. **State the Law Illustrated by These Combinations:** - The law illustrated by these chemical combinations is the **Law of Multiple Proportions**, which states that when two elements combine in different ways to form different compounds, the ratios of the masses of one element that combine with a fixed mass of the other element can be expressed as simple whole numbers. ### Final Answer: The law illustrated by these chemical combinations is the **Law of Multiple Proportions**.
To solve the problem, we need to analyze the two sets of combinations of sulfur and oxygen and identify the law that governs these combinations. ### Step-by-Step Solution: 1. **Identify the Masses of Sulfur and Oxygen in the First Combination:** - In the first case, we have: - Mass of sulfur (S) = 3.2 g - Mass of oxygen (O) = 3.2 g ...
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