The answer is Argon (Ar).
Answer:
0.78 M
Explanation:
First, we need to know which is the value of Kc of this reaction. In order to know this, we should take the innitial values of N2, O2 and NO and write the equilibrium constant expression according to the reaction. Doing this we have the following:
N2(g) + O2(g) <------> 2NO(g) Kc = ?
Writting Kc:
Kc = [NO]² / [N2] * [O2]
Replacing the given values we have then:
Kc = (0.6)² / (0.2)*(0.2)
Kc = 9
Now that we have the Kc, let's see what happens next.
We add more NO, until it's concentration is 0.9 M, this means that we are actually altering the reaction to get more reactants than product, which means that the equilibrium is being affected. If this is true, in the reaction when is re established the equilibrium, we'll see a loss in the concentration of NO and a gaining in concentrations of the reactants. This can be easily watched by doing an ICE chart:
N2(g) + O2(g) <------> 2NO(g)
I: 0.2 0.2 0.9
C: +x +x -2x
E: 0.2+x 0.2+x 0.9-2x
Replacing in the Kc expression we have:
Kc = [NO]² / [N2] * [O2]
9 = (0.9-2x)² / (0.2+x)*(0.2+x) ----> (this can be expressed as 0.2+x)²
Here, we solve for x:
9 = (0.9-2x)² / (0.2+x)²
√9 = (0.9-2x) / (0.2+x)
3(0.2+x) = 0.9-2x
0.6 + 3x = 0.9 - 2x
3x + 2x = 0.9 - 0.6
5x = 0.3
x = 0.06 M
This means that the final concentration of NO will be:
[NO] = 0.9 - (2*0.06)
[NO] = 0.78 M
We can’t answer this question without any information. There is no explanation of the lab, nor is there any data.
Answer:
Ca (s) + 2H₂O (l) → Ca(OH)₂ (aq) + H₂ (g)
Explanation:
When solid calcium reacts with water, it produces the correspondent hydroxid and hydrogen gas.
The hydroxid which is produced, is the calcium hydroxid which is a strong base, that's why you talk about a highly alkaline solution.
Ca (s) + 2H₂O (l) → Ca(OH)₂ (aq) + H₂ (g)
Calcium hydroxide is a strong base, that dissociates in water, as this:
Ca(OH)₂ → Ca²⁺ (aq) + 2OH⁻ (aq)
It's a basic solution, is providing hydroxyl ions to the medium
Answer: orbitals supernumerary
Explanation:
