iamspiderman
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Chlorophile
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(Original post by iamspiderman)
Attachment 282768
Don't understand how to work out this
Question?? :confused:
The question is asking you to work out the enthalpy change for the given equation, which essentially means work out the enthalpy change in J/mol. To start off, you'll want to work out the enthalpy change for the experiment using Q=mc \Delta T.
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iamspiderman
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(Original post by iamspiderman)
Ok thanks
There is no mass given so would I need to divide the 2.00 mol dm-3 by the molar mass of cuso4 to get it?
We're not given the mass but we can work it out. We're given the volume of copper sulfate solution (100ccm) and the density (1g/ccm) and you can work out the mass from this.
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iamspiderman
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(Original post by iamspiderman)
Ok so the mass is 100g
So it will be 100 x 4.18 x 45 = 18,810 ?
Yes, that's the \Delta H for the experiment. You now need to work it out in terms of J/mol.
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iamspiderman
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Borek
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There was an excess of Mg, so you are limited by the amount of copper sulfate. How many moles of copper sulfate in 100 mL of 2.0 M solution?
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iamspiderman
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Yes, 0.2 moles. Now just calculate how much heat would be released per mole of copper sulfate reacting.
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iamspiderman
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Yes.
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