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A 59.4 g sample of the compound X,O, contains 14.4 g of oxygen atoms. What is the molar mass of element X? molar mass of X: 135 g/mol Incorrect

A 59.4 g sample of the compound X,O, contains 14.4 g of oxygen atoms. What is the molar mass of element X? molar mass of X: 135 g/mol Incorrect

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I tried it but I get lost midway the equation.
**Problem Description:** A 59.4 g sample of the compound \(X_4O_6\) contains 14.4 g of oxygen atoms. What is the molar mass of element X? **Input Section:** - Molar mass of X: [Input box where a value can be filled in; example given is 135] **Feedback:** - Incorrect (displayed in red under the input box) **Explanation:** To solve this problem, one can deduce the following steps: 1. **Determine the mass of X in the compound:** - Total mass of sample = 59.4 g - Mass of oxygen in the sample = 14.4 g - Mass of X in the sample = 59.4 g - 14.4 g = 45 g 2. **Calculate the moles of oxygen:** - Molar mass of oxygen (O) = 16 g/mol - Moles of oxygen = 14.4 g / 16 g/mol = 0.9 mol 3. **Find the moles of the compound \(X_4O_6\):** - In \(X_4O_6\), the moles of oxygen are part of \(O_6\) - Therefore, moles of \(X_4O_6\) = moles of \(O_6\) / 6 = 0.9 mol / 6 = 0.15 mol 4. **Calculate the molar mass of X:** - For each \(X_4O_6\), there are 4 X atoms. - Moles of X = 0.15 mol * 4 = 0.6 mol - Molar mass of X = mass of X / moles of X = 45 g / 0.6 mol = 75 g/mol Thus, the correct answer for the molar mass of element X is 75 g/mol, not 135 g/mol as initially inputted.
Transcribed Image Text:**Problem Description:** A 59.4 g sample of the compound \(X_4O_6\) contains 14.4 g of oxygen atoms. What is the molar mass of element X? **Input Section:** - Molar mass of X: [Input box where a value can be filled in; example given is 135] **Feedback:** - Incorrect (displayed in red under the input box) **Explanation:** To solve this problem, one can deduce the following steps: 1. **Determine the mass of X in the compound:** - Total mass of sample = 59.4 g - Mass of oxygen in the sample = 14.4 g - Mass of X in the sample = 59.4 g - 14.4 g = 45 g 2. **Calculate the moles of oxygen:** - Molar mass of oxygen (O) = 16 g/mol - Moles of oxygen = 14.4 g / 16 g/mol = 0.9 mol 3. **Find the moles of the compound \(X_4O_6\):** - In \(X_4O_6\), the moles of oxygen are part of \(O_6\) - Therefore, moles of \(X_4O_6\) = moles of \(O_6\) / 6 = 0.9 mol / 6 = 0.15 mol 4. **Calculate the molar mass of X:** - For each \(X_4O_6\), there are 4 X atoms. - Moles of X = 0.15 mol * 4 = 0.6 mol - Molar mass of X = mass of X / moles of X = 45 g / 0.6 mol = 75 g/mol Thus, the correct answer for the molar mass of element X is 75 g/mol, not 135 g/mol as initially inputted.
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