24. A laboratory chemist wants to produce 25.0 g NO2 by the following reactions. If the
1 answer:
The amount of N2O5 to start with would be 35.79 grams
<h3>Stoichiometric calculations</h3>
From the balanced equation of the reactions:
Mole ratio of N2O5 and NO2 = 1:2
Since the reaction's actual yield is 82%, the theoretical yield would be: 25 x 100/82 = 30.49 grams
Mole of 25 g NO2 = 30.49/46
= 0.66 mole
Equivalent mole of N2O5 = 0.54/2 mole
= 0.33 moles
Mass of 0.27 mole N2O5 = 0.33 x 108.01
= 35.79 grams
More on stoichiometric calculations can be found here: brainly.com/question/8062886
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Answer:
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Explanation:
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In this case, according to the given information, it turns out possible for us to calculate the absorbed heat by considering this is a process involving sensible heat associated to the vaporization of water, which is isothermic and isobaric; and thus, the heat of vaporization of water, with a value of about 2259.36 J/g, is used as shown below:
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