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A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and...

A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 °C?

Solutions

Expert Solution

weight of BaCl2·2H2O    = 8.4g

gram molecular weight of BaCl2·2H2O    = 244.257g/mole

no of moles of BaCl2·2H2O   = W/G.M.Wt

                                              = 8.4/244.257 = 0.0344 moles

1 mole of BaCl2. 2H2O contains 2 moles of H2O

0.0344 moles of BaCl2.2H2O contains = 2*0.0344/1 = 0.0688 moles of H2O

n = 0.0688moles

P   = 1atm

T   = 100+273 = 373K

PV   = nRT

V    = nRT/P

        = 0.0688*0.0821*373/1   = 2.1 L

The volume of steam = 2.1L >>>>answer

queen_honey_blossom answered 2 years ago
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