An element X forms an iodide (XI 3 ) and a chloride (XCl 3 ). The iodide is quantitatively converted to the chloride when it is heated in a stream of chlorine: 2 XI 3 + 3 Cl 2 → 2 XCl 3 + 3 I 2 If 0.5000 g of XI 3 is treated with chlorine, 0.2360 g of XCl 3 is obtained. (a) Calculate the atomic weight of the element X. (b) Identify the element X.

Hi everyone here we have a question telling us a medal from group to a forms of bromide with the formula M B R two. And chloride with the formula M C L. To the bromide can be converted into chloride. When reacted with chlorine gas. And it gives us the reaction M BR two plus chlorine form M C L two plus browning. When a 0.242554 g sample of M B R two is reacted with excess chlorine, 0.1321 g of M C L two is produced. And the question is, what is the atomic weight of the metal? M So because of the equation, we know that our Ratio of MBR two To MCL two Is 1 - one. So our moles of NBR two equals the mass of NBR two Over the formula mass of NBR two. Likewise, the moles of MCL two is going to equal the mess of MCL two over the formula mass By the MCL two. So our formula mass of MBR two equals M plus two times the molar mass of roaming because there's two of them, which is 79. g per mole. And likewise the formula mass of MCL two equals M the Mueller massive M plus two times the molar mass of chlorine, which is 35.45 to 7 graham's Permal. So the moles of NBR two Equals 0. Times in Plus two times 79.904. The moles of MCL two Equals 0.1321. I'm sorry, divided by, divided by M Plus two times 35.45 - seven. So they equal each other. So we have 0.2554, divided by M Plus 159. equals 0. over, M. 70.9054. So we end up with zero .2554. M plus 0. Times 70. Equals 0.1321. M plus 0.132, one times 159.808. So 0.1233, M Equals 3.00139764. Which means m equals 3.00139764, Divided by 0.1233. So m equals 24. grams per mole. And that is our final answer. Thank you for watching. Bye

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 15th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 96a,b

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Chapter 3, Problem 96a,b

An element X forms an iodide (XI₃) and a chloride (XCl₃). The iodide is quantitatively converted to the chloride when it is heated in a stream of chlorine: 2 XI₃ + 3 Cl₂ → 2 XCl₃ + 3 I₂ If 0.5000 g of XI₃ is treated with chlorine, 0.2360 g of XCl₃ is obtained. (a) Calculate the atomic weight of the element X. (b) Identify the element X.

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Identify the chemical reaction: \(2 \text{XI}_3 + 3 \text{Cl}_2 \rightarrow 2 \text{XCl}_3 + 3 \text{I}_2\).

Determine the molar mass of \(\text{XI}_3\) and \(\text{XCl}_3\) using the given masses and the stoichiometry of the reaction.

Use the mass of \(\text{XI}_3\) (0.5000 g) and \(\text{XCl}_3\) (0.2360 g) to set up a ratio based on the stoichiometry of the reaction.

Calculate the molar mass of \(\text{XI}_3\) and \(\text{XCl}_3\) using the atomic masses of iodine and chlorine, and the unknown atomic mass of \(X\).

Solve the equations to find the atomic weight of element \(X\) by equating the molar masses derived from the given data.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry is essential for relating the masses of XI3 and XCl3 to find the atomic weight of element X.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic weights of all atoms in a molecule. To find the atomic weight of element X, one must first determine the molar masses of XI3 and XCl3, which will help in calculating the mass contribution of X in the reaction.

Conservation of Mass

The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. This principle allows chemists to account for all reactants and products in a reaction. In this problem, the total mass of XI3 before the reaction must equal the total mass of XCl3 and I2 produced, which is crucial for calculating the atomic weight of X based on the given masses.

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