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Alekssandra [29.7K]
3 years ago
8

A certain chemical reaction releases 36.2 kJ/g of heat for each gram of reactant consumed. How can you calculate what mass of re

actant will produce 1360 J of heat?
Chemistry
1 answer:
Lilit [14]3 years ago
5 0

Answer:

0.038 g of reactant

Explanation:

Data given:

Heat release for each gram of reactant consumption = 36.2 kJ/g

mass of reactant that release 1360 J of heat = ?

Solution:

As  36.2 kJ of heat release per gram of reactant consumption so first we will convert KJ to J

As we know

1 KJ = 1000 J

So

36.2 kJ = 36.2 x 1000 = 36200 J

So it means that in chemical reaction 36200 J of heat release for each gram of reactant consumed so how much mass of reactant will be consumed if 1360 J heat will release

Apply unity formula

                 36200 J of heat release ≅ 1 gram of reactant

                 1360 J of heat release ≅ X gram of reactant

Do cross multiplication

              X gram of reactant = 1 g x 1360 J / 36200 J

              X gram of reactant = 0.038 g

So 0.038 g of reactant will produce 1360 J of heat.

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Answer:

Explanation:

Elements on the right side of the periodic table are very likely to form negative ions -- all of those except elements in the 8th or 18th column (depending on how your periodic table is numbered).

K and Mg are on the left side, so they will not form negative ions.

They give up 1 (for K) electron and 2 (for Mg) electrons which will leave plus charges for the ions.

On the other hand S and I are on the right side of the periodic table. They will take on electrons and hence be charged with a minus.

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2 years ago
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Example:

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3 years ago
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What is the total number of moles of the reactants in the following reaction?
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Assuming that 2H2O(l) is the product, the reactants would be 2H2(g) and O2(g). The number of moles in the reactants would be 2 moles of H2 and 1 mole of O2.
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sineoko [7]

kilo is 1,000 times the base unit <em>(tip for remembering: think money, 1k is 1,000)</em>

centi is 1/100 of the base unit <em>(tip for remembering: cent = 100)</em>

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