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A 1.526-g sample of a hydrate of magnesium sulfate (MgSO4∙xH2O) is heated in a crucible, cooled, and weighed. The final constant mass reached is 0.748 g. Which of the following options correctly interpret these data? (Select all that apply.) The sample contained 0.778 g of H2O. The sample contained 49.02% H2O by mass. There are 5 moles of H2O per mole of MgSO4. The sample contained 4.32 x 10-2 moles of H2O. The mole ratio of Mg2+ to H2O in this compound is 1:7.

A 1.526-g sample of a hydrate of magnesium sulfate (MgSO4∙xH2O) is heated in a crucible, cooled, and weighed. The final constant mass reached is 0.748 g. Which of the following options correctly interpret these data? (Select all that apply.) The sample contained 0.778 g of H2O. The sample contained 49.02% H2O by mass. There are 5 moles of H2O per mole of MgSO4. The sample contained 4.32 x 10-2 moles of H2O. The mole ratio of Mg2+ to H2O in this compound is 1:7.

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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A 1.526-g sample of a hydrate of magnesium sulfate (MgSO4∙xH2O) is heated in a crucible, cooled, and weighed. The final constant mass reached is 0.748 g. Which of the following options correctly interpret these data? (Select all that apply.)

The sample contained 0.778 g of H2O.

The sample contained 49.02% H2O by mass.

There are 5 moles of H2O per mole of MgSO4.

The sample contained 4.32 x 10-2 moles of H2O.

The mole ratio of Mg2+ to H2O in this compound is 1:7.

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