Answer:
Step 3
Explanation:
I am back sorry it took me so long, I believe its Step 3 because that's were you chose your strategy, you use it in Step 4, but if its not Step 3 its Step 4
1. identifying
problem solving step: 1)__ the problem is most difficult: not in habit of asking what the problem really is; in the habit of reacting or giving up
2. representing
problem solving step: 2) __ the problem: abstract or external representation
3. strategy
problem solving step: 3) selecting an appropriate __; trial and error vs means-ends analysis
4. implementing
problem solving step: 4) __ the strategy; dependent on previous steps
Answer:
The left side equation is:
![Ka = \frac{[CH_{3}COO^{-}] [H_{3}O^{+}]}{[HCH_{3}COO] [H_{2}O]}](https://tex.z-dn.net/?f=Ka%20%3D%20%5Cfrac%7B%5BCH_%7B3%7DCOO%5E%7B-%7D%5D%20%5BH_%7B3%7DO%5E%7B%2B%7D%5D%7D%7B%5BHCH_%7B3%7DCOO%5D%20%5BH_%7B2%7DO%5D%7D)
Explanation:
For the reaction of acetic acid HCH3CO2 with the water, The equilibrium constant equation is
The left side of this equilibrium constant equation will be written as shown below:
Answer:
(ii) Ethane and Heptadecane
Explanation:
The separation of all the species listed in the answer options for the question depends on the molar mass of each specie.
Ethane is a low molecular mass gas. It exists in the gaseous state at room temperature. However, heptadecane appears as a liquid because it has a greater relative molecular mass.
It is very easily to distinguish between the gas, ethane and the liquid heptadecane which is a high molecular mass alkane, hence the answer.
Answer:
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Explanation:
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Answer:
Solid ionic compounds do not conduct electricity because the ions are held firmly in place. The ions cannot move to conduct the electric current. But when an ionic compound melts, the charged ions are free to move. Therefore, molten ionic compounds do conduct electricity.
