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kumpel [21]
3 years ago
9

During a lab, you heat 1.04 g of a niso4 hydrate over a bunsen burner. after heating, the final mass of the dehydrated compound

is 0.61 g. determine the formula of the hydrate and also give the full name of the hydrate.
Chemistry
1 answer:
slamgirl [31]3 years ago
5 0
The difference between the initial mass (1.04 g) and the final mass (0.61g) is the mass of water present in the sample:

1.04 g - 0.61 g = 0.43 g

Divide by the molar mass of water: 18.01 g / mol to obtain the number of moles of water:

0.43 g / 18.01 g / mol = 0.0239 moles

Calculate the number of moles of dehydrated NiSO4

Number of moles = mass in grams / molar mass

molar mass of NiSO4 = 154.75 g/mol

number of moles NiSO4 = 0.61 g / 154.75 g/mol = 0.00394 moles

Now determine the molar ratio water to NiSO4: 0.0239 / 0.00394 = 6.07 ≈ 6

Then, the formula of the hydrate product is NiSO4 · 6 H2O.

Use the prefix hexa (6) to name the compound: Nickel(II) sulfate hexadydrate
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Using PV = nRT, we can calculate the moles of the sample.
874 mmHg = 116,524 Pa
n = PV/RT
n = 116,524 x 294 x 10⁻⁶ / 8.314 x (140 + 273)
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moles = mass / Mr
Mr = 0.271/9.98 x 10⁻³
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1 mole produces 2 moles of CO₂, so 3 moles will produce 6 moles CO₂
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