Answer:
H2
Explanation:
In the first place it is necessary to consider that these two elements will be their diatomic form initially, that is, H2 and N2.
first we should check the equilibrium constant Kp tables in this case at a temperature of 3000K
Value for dissociation reaction of H2 in Kp = -3.685
Value for dissociation reaction of N2 in Kp = -22.359
Equilibrium constant for H2 dissociation is higher than N2 dissociation. so for this comparation H2 is more likely to dissociate.
Answer:
She gave them bottles with labels showing the brands
Explanation:
the teens could have been biased due to knowing the brand. It would have been more reliable if the label was covered or removed.
Answer:
- Molar mass of Ca₃(PO₄)₂ = 310.18 g/mol
- 934.32 g Ca₃(PO₄)₂ = 3.01 moles Ca₃(PO₄)₂
Explanation:
The<em> molar mass </em>(MM)<em> of Ca₃(PO₄)₂</em> can be calculated as follows:
- MM of Ca₃(PO₄)₂ = (MM of Ca)*3 + [(MM of P) +(MM of O)*4]*2
- MM of Ca₃(PO₄)₂ = 310.18 g/mol
Now we can <u>convert 934.32 g of Ca₃(PO₄)₂ into moles</u>:
- 934.32 g ÷ 310.18 g/mol = 3.01 moles
Answer:
A flame test could help by seeing what things it could catch on fire from or the things that could happen with acids etc. I would test the medicine by asking someone who has had it in their life, asking doctors or I would maybe use it myself maybe. (I don’t know about c, sooo sorry)
The question is incomplete, the complete question is:
The reaction:
SO_2 (g) + 2 H2S (g) <=> 3 S(s) + 2 H2O(g)
is the basis of a suggested method for removal of {SO2} from power-plant stack gases.
Kp = 8×10^15
In principle, is this reaction a feasible method of removing SO_2 from power-plant emissions?
1. No; the reaction is highly spontaneous at 298 K, but a significant amount of SO2 will remain at equilibrium.
2. Yes; the reaction is highly spontaneous at 298 K, even though a significant amount of SO2 will remain at equilibrium.
3. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium.
4. No; the reaction is not spontaneous at 298 K, even though almost no SO2 will remain at equilibrium.
5. No; the reaction is not spontaneous at 298 K and a significant amount of SO2 will remain at equilibrium.
Answer:
3. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium
Explanation:
Looking at the Kp of the of the reaction, we expect that almost no sulphur IV oxide should remain at equilibrium. The Kp has a a large value of 8×10^15 which indicates that the reaction should proceed to completion. The reaction is also spontaneous at 298K.
