From Mastering Chemistry 11.137 Homework: Treatment of 1.385 g of an unknown met

Question

From Mastering Chemistry 11.137 Homework:

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 ?Cand 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HClthen gave a white crystalline compound, MClx. After dissolving the compound in 25.0g of water, the melting point of the resulting solution was -3.53?C.

How many moles of H2 gas are evolved?

What mass of MCl is formed?

What is the molality of particles (ions) in the solution of MCl?

How many moles of ions are in the solution?

What is the molecular mass of MCl?

What is the formula of MCl?What is the identity of the metal M?

Explanation / Answer

Dont know the moles of H2 gas envolved but here is the answers to the rest

a) 1.58x10^-2 mol

b) 0.0316 mol

c) 1.90m

d) 4.75x10^-2

e)157.5

f)SrCl2 -the formula of MCl
Sr-the identity of the metal M

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