Answer:
The independent variable is the effect of tempeture on the rate of photosynthesis
Answer:
pOH = 0.3
Explanation:
As KOH is a strong base, the molar concentration of OH⁻ is equal to the molar concentration of the solution. That means that in this case:
With that information in mind we can<u> calculate the pOH </u>by using the following formula:
Answer:
Cr₂S₃
Explanation:
From the question given above, the following data were obtained:
Mass of chromium (Cr) = 0.67 g
Mass of chromium sulfide = 1.2888 g
Empirical formula =?
Next, we shall determine the mass of sulphur (S) in the compound. This can be obtained as follow:
Mass of chromium (Cr) = 0.67 g
Mass of chromium sulfide = 1.2888 g
Mass of sulphur (S) =?
Mass of S = (Mass of chromium sulfide) – (Mass of Cr)
Mass of S = 1.2888 – 0.67
Mass of S = 0.6188 g
Finally, we shall determine the empirical formula of the compound. This can be obtained as follow:
Mass of Cr = 0.67 g
Mass of S = 0.6188 g
Divide by their molar mass
Cr = 0.67 / 52 = 0.013
S = 0.6188 / 32 = 0.019
Divide by the smallest
Cr = 0.013 / 0.013 = 1
S = 0.019 / 0.013 = 1.46
Multiply by 2 to express in whole number
Cr = 1 × 2 = 2
S = 1.46 × 2 = 3
Therefore, the empirical formula of the compound is Cr₂S₃
Explanation:
The given reaction will be as follows.
............. (1)
= ![[Ag^{+}][Cl^{-}] = 1.8 \times 10^{-10}](https://tex.z-dn.net/?f=%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D%20%3D%201.8%20%5Ctimes%2010%5E%7B-10%7D)
Reaction for the complex formation is as follows.
![Ag^{+}(aq) + 2NH_{3}(aq) \rightleftharpoons [Ag(NH_{3})_{2}]^{+}(aq)](https://tex.z-dn.net/?f=Ag%5E%7B%2B%7D%28aq%29%20%2B%202NH_%7B3%7D%28aq%29%20%5Crightleftharpoons%20%5BAg%28NH_%7B3%7D%29_%7B2%7D%5D%5E%7B%2B%7D%28aq%29)
........... (2)
= ![\frac{[Ag(NH_{3})_{2}]}{[Ag^{+}][NH_{3}]^{2}} = 1.0 \times 10^{8}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BAg%28NH_%7B3%7D%29_%7B2%7D%5D%7D%7B%5BAg%5E%7B%2B%7D%5D%5BNH_%7B3%7D%5D%5E%7B2%7D%7D%20%3D%201.0%20%5Ctimes%2010%5E%7B8%7D)
When we add both equations (1) and (2) then the resultant equation is as follows.
![AgCl(s) + 2NH_{3}(aq) \rightarrow [Ag(NH_{3})_{2}]^{+}(aq) + Cl^{-}(aq)](https://tex.z-dn.net/?f=AgCl%28s%29%20%2B%202NH_%7B3%7D%28aq%29%20%5Crightarrow%20%5BAg%28NH_%7B3%7D%29_%7B2%7D%5D%5E%7B%2B%7D%28aq%29%20%2B%20Cl%5E%7B-%7D%28aq%29)
............. (3)
Therefore, equilibrium constant will be as follows.
K = 
= 
= 
Since, we need 0.010 mol of AgCl to be soluble in 1 liter of solution after after addition of 
for complexation. This means we have to set
![[Ag^{+}]](https://tex.z-dn.net/?f=%5BAg%5E%7B%2B%7D%5D)
= ![[Cl^{-}]](https://tex.z-dn.net/?f=%5BCl%5E%7B-%7D%5D)
= 
= 0.010 M
For the net reaction,
Initial : 0.010 x 0 0
Change : -0.010 -0.020 +0.010 +0.010
Equilibrium : 0 x - 0.020 0.010 0.010
Hence, the equilibrium constant expression for this is as follows.
K = ![\frac{[Ag(NH_{3})^{+}_{2}][Cl^{-}]}{[NH_{3}]^{2}}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BAg%28NH_%7B3%7D%29%5E%7B%2B%7D_%7B2%7D%5D%5BCl%5E%7B-%7D%5D%7D%7B%5BNH_%7B3%7D%5D%5E%7B2%7D%7D)
= 
x = 0.0945 mol
or, x = 0.095 mol (approx)
Thus, we can conclude that the number of moles of needed to be added is 0.095 mol.
