in experiment 2.4 g of iron oxide

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In an experiment, 2.4 g of Iron oxide on reduction with Hydrogen yields 1.68 g of Iron. In another experiment, 2.9 g of Iron oxide give 2.03 g of Iron on reduction with Hydrogen. Show that the above data illustrates the law of constant proportion.

To demonstrate that the given data illustrates the law of constant proportion, we will analyze the mass ratios of iron and oxygen produced from the reduction of iron oxide in both experiments. 1. Identify the Given Data: - Experiment 1: - Mass of Iron Oxide (FeO) = 2.4 g - Mass of Iron (Fe) produced = 1.68 g - Experiment 2: - Mass of Iron Oxide (FeO) = 2.9 g - Mass of Iron (Fe) produced = 2.03 g 2. Calculate the Mass of Oxygen in Each Experiment: - For Experiment 1: Mass of Oxygen = Mass of Iron Oxide − Mass of Iron = 2.4 g − 1.68 g = 0.72 g - For Experiment 2: Mass of Oxygen = Mass of Iron Oxide − Mass of Iron = 2.9 g − 2.03 g = 0.87 g 3. Determine the Mass Ratios of Iron to Oxygen: - For Experiment 1: Ratio of Iron to Oxygen = Mass of Iron Mass of Oxygen = 1.68 g 0.72 g = 2.33 - For Experiment 2: Ratio of Iron to Oxygen = Mass of Iron Mass of Oxygen = 2.03 g 0.87 g = 2.33 4. Compare the Ratios: - Both experiments yield the same ratio of iron to oxygen: - Experiment 1: 2.33 - Experiment 2: 2.33 5. Conclusion: - Since the ratio of the masses of iron to oxygen remains constant (2.33) in both experiments, this illustrates the law of constant proportion. This law states that in a given compound, the elements are always present in a definite mass ratio, regardless of the source or method of preparation.

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SOME BASIC CONCEPTS OF CHEMISTRY

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In an experiment 2.4g of iron oxide in reduction with hydrogen gave 1.68 g of iron. in another experimet, 2.7 g of iron oxide gave 1.89 g of iron on reduction. which law is illustrated from the above data.

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In an experiment, 2.4 g of iron oxide on reduction with hydrogen gave 1.68 g of iron. In another experiment, 2.7 g of iron oxide gave 1.89 g of iron on reduction. Which law is illustrated from the above data?

Q. In an experiment, 2.4 g of iron oxide on reduction with hydrogen gave 1.68 g of iron. In another experiment, 2.7 g of iron oxide gave 1.89 g of iron on reduction. Which law is illustrated from the above data?

Law of constant proportions, law of multiple proportions, law of reciprocal proportions, law of conservation of mass, in first experiment, mass of iron oxide = 2.4 g mass of iron = 1.68 g mass of oxygen = 2.4 − 1.68 = 0.72 ratio of masses of iron and oxygen = 0.72 1.68 = 7 : 3 in second experiment, mass of iron oxide = 2.7 g mass of iron = 1.89 g mass of oxygen = 2.7 − 1.89 = 0.81 ratio of masses of iron and oxygen = 0.81 1.89 = 7 : 3 the same ratio confirms that these experiments clarify law of constant proportions..