Arrhenius concept just states that if a solution dissociates and forms H+ ions then its an acid, but if it dissociates and forms OH- than it's a base.
So, HNO3 would be classified as an acid
The given question is incomplete. The complete question is:
The enthalpy change, ΔH, for a reaction at constant pressure is defined as: ΔH = ΔE + PΔV. For which of the following reactions will ΔH be approximately equal to ΔE? Select all that apply. Group of answer choices
None of the above
Answer:
Explanation:
Relation of with is given by the formula:
as
Where,
= enthalpy change
= internal energy change
R = Gas constant
T = temperature
= change in number of moles of gas particles = 
1. For
2. For 
3.
Thus for reactions 2 and 3, ΔH be approximately equal to ΔE
Answer:
1.12x10²³ atoms of F
Explanation:
A molecule is a group of 2 or 3 atoms that are bonded by electrostatic charges.
In 1 molecule of MgF2 there are 2 atoms of fluorine and 1 atom of magnesium.
Thus, there are 2 atoms of fluorine per molecule of MgF2. In 5.6x10²² molecules:
5.6x10²² molecules MgF2 * (2 atoms Fluorine / 1 molecule MgF2) =
<h3>1.12x10²³ atoms of F</h3>
Answer:
Smaller
Explanation:
Though, your question is not too clear but base on my understanding, I have the following explanation;
The angle in the bromine-oxygen bonds will be smaller than the ideal angle, say for example, if the ideal angle is 120°, the actual angle of bromine-oxygen bonds will have lesser value because of the absence of lone pairs of electrons from the central atom in the ion. This will tend to squeeze the two single bond that exist before causing lesser angle.
Hello,
Here is your answer:
The proper answer to this question is option B "a data table". Data tables are not examples of scientific models.
Your answer is B.
If you need anymore help feel free to ask me!
Hope this helps!
