We must __________ forces to calculate net force if the forces are going in OPPOSITE directions.
1 answer:
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Hello!
To find electron configuration for Idoine we need to understand the following steps:
- Finding the Atom's Atomic Number (tells us the specific number of electrons)
- Determining the Charge of the Atom
- Understanding the orbitals (Set S [Contains 2], P [Contains 3, Holds 6], D [Contains 5, Holds 10], F [Contains 7, Holds 14], and there are some theoritical ones.) [Overall the sets go SPDFGHIK
- Understanding notations in configuartion. The notations display the number of electrons in the atom and set.
In this case, for Iodine. If we follow these rules we can see that the electron configuration is [Kr] 4d^10 5s^2 5p^5. We use Krytpon in front because that is the last full and stable noble gas before this particular element. Atoms are just trying to be stable so the goal is to achieve that full shell.
Answer : The amount of heat released in the combustion is, 209.5 kJ
Explanation :
First we have to calculate the moles of Al and .
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction will be:
From the balanced reaction we conclude that
As, 3 mole of react with 4 mole of
So, 0.188 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
From the reaction, we conclude that
As, 3 mole of react to give 2 mole of
So, 0.188 moles of react to give
moles of
Now we have to calculate the amount of heat released in the combustion.
As, 1 mole of releases amount of heat = 1676 kJ
So, 0.125 mole of releases amount of heat =
Thus, the amount of heat released in the combustion is, 209.5 kJ
Answer:
Explanation:
Hello!
In this case, since the Gibbs free energy of any process is related with the enthalpy change, temperature and entropy change as shown below:
For a chemical reaction it is simply modified to:
Thus, since the enthalpy of reaction is given as -304.2 kJ and the entropy as -414.2 J/K (-0.4142 kJ/K), at 775 K the Gibbs free energy of reaction turns out:
Whose result means this is a nonspontaneous reaction.
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