Answer:
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Explanation:
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The correct answer is reaction 2 most likely occurred in their experiment.
So the given two reactions are as follows:
1) Au³⁺(aq) + Co(s) --> Au(s) + Co³⁺(aq)
2) 2Au³⁺(aq) + 3Co(s) --> 2Au(s) + 3Co³⁺(aq)
Mass of Co = 6.087 g
Molar mass of Co = 58.933 g/mol
Moles of Co = = 0.1032
Mass of Au = 13.572 g
Molar mass of Au = 196.967 g/mol
Moles of Au = = 0.069
Now based on reaction 1) the molar ratio between Co and Au is 1:1
So as per this reaction 0.1032 moles of Co would produce 0.1032 mole of Au
Again based on reaction 2) the molar ratio between Co and Au is 3:2
So as per this reaction 0.1032 moles of Co would produce mole of Au
or, As per the second reaction 0.1032 moles of Co would produce 0.0688 moles of Au
<u>Answer:</u> The enthalpy change of the reaction is 58 kJ.
<u>Explanation:</u>
Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as
The equation used to calculate enthalpy change is of a reaction is:
For the given chemical reaction:
The equation for the enthalpy change of the above reaction is:
We are given:
Putting values in above equation, we get:
Hence, the enthalpy change of the reaction is 58 kJ.
Answer:
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