Answer :
Explanation :
The aluminium and fluorine react to give ionic compound aluminium fluoride.
Aluminium has 1 valence electrons in their shell and fluorine has 7 valence electrons in their shell.
For the complete octet, both aluminium and fluorine exchange valence electrons to form an ionic compound.
The aluminium donates its three valence electrons to three fluorine atoms and they form one
and three
ions.
Electron transfer image is shown below.
Answer:
See explanation
Explanation:
Qualitative analysis in chemistry is a method used to determine the ions present in a solution chiefly by means of chemical reactions.
In this case, I suspect the presence of silver ions and/or barium ions. The first step is to add dilute HCl. This will lead to the precipitation of the silver ion as AgCl. If a white precipitate is formed upon addition of HCl then Ag^+ is present in the solution.
Secondly, I add a carbonate such as NH4CO3(aq). This will cause the barium ions to become precipitated as barium carbonate. Hence, the formation of a white precipitate when NH4CO3(aq) is added to the solution indicates the presence of barium ion in the solution.
The first one a neutral neutron strikes a large neutral nucleus
Answer: Option C) 9.5
Explanation:
Given that,
pOH of solution = ?
pH of solution = 4.5 (it is an acidic solution because any pH values less than 7.0 is said to be acidic)
Recall that pH is the negative logarithm of hydrogen ion concentration in the solution while pOH is the negative logarithm of hydroxide ion concentration in the solution.
Hence, pH + pOH = 14
4.5 + pOH = 14
pOH = 14 - 4.5
pOH = 9.5
Thus, the pOH of the same solution is 9.5
Answer:
Part A
![rate= 4.82*10^{-3}s^{-1} * [N2O5]](https://tex.z-dn.net/?f=rate%3D%204.82%2A10%5E%7B-3%7Ds%5E%7B-1%7D%20%2A%20%5BN2O5%5D)
Part B

Explanation:
Part A
<em>The rate law is the equation that relates the rate of the reaction, the kinetic constant and the concentration of the reactant or reactants.</em>
For the given chemical reaction we can write a general expression for the rate law as follows:
![rate= k * [N2O5]^{x}](https://tex.z-dn.net/?f=rate%3D%20k%20%2A%20%5BN2O5%5D%5E%7Bx%7D)
where k is the rate constant and x is the order of the reaction with respect of N2O5 concentration. Particularly, <em>a first order reaction kinetics indicate that the rate of the reaction is directly proportional to the concentration of only one reactant</em>. Then x must be 1.
Replacing the value of the rate constant given in the text we can arrive to the following expression for the rate law:
![rate= 4.82*10^{-3}s^{-1} * [N2O5]](https://tex.z-dn.net/?f=rate%3D%204.82%2A10%5E%7B-3%7Ds%5E%7B-1%7D%20%2A%20%5BN2O5%5D)
Part B
Replacing the value of the concentration of N2O5 given, we can get the rate of reaction:

