A chemist measures the energy change ?H during the following reaction:
1 answer:
Answer:
(A) endothermic
(A) Yes, absorbed
Explanation:
Let's consider the following thermochemical equation.
2 Fe₂O₃(s) ⇒ 4 FeO(s) + O₂(g) ΔH = 560 kJ
Since ΔH > 0, the reaction is endothermic.
We can establish the following relations:
- 560 kJ are absorbed when 2 moles of Fe₂O₃ react.
- The molar mass of Fe₂O₃ is 160 g/mol.
Suppose 66.6 g of Fe₂O₃ react. The heat absorbed is:
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Answer:- 0.158 moles
Solution:- Moles are calculated on dividing the grams by the molar mass.
25.0 grams of are given and we are asked to calculate the moles.
For this we need the molar mass so let's calculate it first.
Molar mass is the sum of atomic masses of all the atoms present in the molecule.
Molar mass =
= 158.036 gram per mol
Now, we will divide the given grams by molar mass to get the moles and the set is shown as:
=
So, there are 0.158 moles of .
Answer:
Explanation:
Hello,
In this case, for the calculation of the half-life for the mentioned reaction we first must realize that considering the units of the rate constant and the form of the rate law, it is a second-order reaction, therefore, the half-life expression is:
Therefore, we obtain:
Regards.