Another chemistry question
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This post was last edited by xwtsq on 2009-8-11 at 21:41. The title is as follows: At 20°C, 10 mL of a 0.1 mol/L Na2SO3 solution and 10 mL of a 0.1 mol/L H2SO4 solution were mixed; after 2 minutes, the solution became noticeably cloudy. It is known that for every 10°C increase in temperature, the rate of a chemical reaction doubles. Therefore, at 50°C, the time required for the same reaction to produce the same level of turbidity is ( ). A 40s B 15s C 48s D 20s The question now is, how do we write the chemical equation for this reaction? Is there a mistake in the title?
1# xwtsq: I’ve forgotten a lot about chemical analysis, but it seems there’s an issue. I remember that in reactions, effective collisions between activated molecules are important; by increasing the temperature, the speed of these activated molecules as well as the speed of all molecules increases. But it shouldn’t be such a simple linear relationship, right? ? ? Na2SO4 + SO2 ↑ + H2O I’m not sure if this is the correct equation. . . . If there are any mistakes or other opinions, please feel free to point them out, dear friends.....
H2SO4 should be H2S; in that case, it should take 15 seconds at 50 degrees
As a supplementary note, the turbidity is due to elemental S.
Haha :lol My equation is wrong. . . . That’s so stupid. The question states that the phenomenon is turbidity. . . .
It seems that Na2SO3 should be sodium thiosulfate; if the reaction holds, the answer should be B
Sodium sulfite and sulfuric acid do not react with each other in theory; is it sodium thiosulfate instead?
Back to floor 6: Your feeling is likely correct, and the answer is also right. This is a question meant for high school students, and upon seeing it, I thought there was an error in its formulation. I flipped through the \"Inorganic Chemistry Series\" books; it seems the title mistakenly lists sodium thiosulfate as sodium sulfite.
The answer is B, right? It seems everyone knows it
This post was last edited by Synthesis GG on 2009-8-17 21:20. A disproportionation reaction requires an intermediate oxidation state; how does this reaction take place?
The title is correct; sulfites undergo a disproportionation reaction of self-redox under the action of strong acids. NA2SO3+H2SO4(4H+)-----NA2SO4+S (solid precipitate)+2H2O