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A 1.00-g sample of magnesium sulfate is dissolved in water, and the water is then evaporated away until the residue is bone dry. If the temperature of the water is kept between 48^∘ C and 69^∘ C, the solid that remains weighs 1.898  g. If the experiment is repeated with the temperature held between 69^∘ C and 100^∘ C, however, the solid has a mass of 1.150  g. Determine how many waters of crystallization per MgSO4 there are in each of these two solids. | Numerade

Consider the following reaction: 2Mg (s) O2 (g) -> 2MgO (s) ΔH = -1203 kJIf 4 moles of magnesium completely react, what is the amount of heat (in kJ) that will be released? (Show calculation set-up)

SOLVED: How much heat is released when 3.5 g of magnesium oxide is produced in the following reaction:8Mg(s) Mg(NO3)2(s) ? Mg3N2(s) 6MgO(s) ?rH = -3884 kJNote: Ignore the significant figures when you answer.

What is formula of magnesium hydroxide   - 72254988

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