Consider the fictional element A (which has a molar mass of 7.00 g/mol) and the fictional element D (which has a molar mass of 13.00 g/mol). Suppose that 16.20 grams of an unknown hydrate of A2D are heated until a constant mass of 5.40 grams is reached. How many waters are in the empirical formula of the hydrate? (For example, if the empirical formula were Na2SO4 ⋅ 10 H2O, your answer would be 10.)
Consider the fictional element A (which has a molar mass of 7.00 g/mol) and the fictional element D (which has a molar mass of 13.00 g/mol). Suppose that 16.20 grams of an unknown hydrate of A2D are heated until a constant mass of 5.40 grams is reached. How many waters are in the empirical formula of the hydrate? (For example, if the empirical formula were Na2SO4 ⋅ 10 H2O, your answer would be 10.)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter10: Solutions
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Problem 16QAP
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Consider the fictional element A (which has a molar mass of 7.00 g/mol) and the fictional element D (which has a molar mass of 13.00 g/mol).
Suppose that 16.20 grams of an unknown hydrate of A2D are heated until a constant mass of 5.40 grams is reached.
How many waters are in the empirical formula of the hydrate? (For example, if the empirical formula were Na2SO4 ⋅ 10 H2O, your answer would be 10.)
Expert Solution
Step 1
Given:
The molar mass of element A and B is 7.00 g/mol and 13.00 g/mol, respectively.
The mass of the unknown hydrate of A2D is 16.20 g.
The final mass obtained is 5.40 g.
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