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Question
Consider the reaction:
\[\ce{6 CO2(g) + 6H2O(l) → C6 H12O6(aq) + 6O2(g)}\]
Why it is more appropriate to write these reaction as:
\[\ce{6CO2(g) + 12H2O(l) → C6 H12O6(aq) + 6H2O(l) + 6O2(g)}\]
Also, suggest a technique to investigate the path of the redox reactions.
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Solution
The process of photosynthesis involves two steps.
Step 1:
H2O decomposes to give H2 and O2.
Step 2:
The H2 produced in step 1 reduces CO2, thereby producing glucose (C6H12O6) and H2O.
\[\ce{6CO_{2(g)} + 12H_{2(g)} -> C_6H_12O_{6(s)} + 6H_2O_{(l)}}\]
Now, the net reaction of the process is given as:
| \[\ce{2H_2O_{(l)} -> 2H_{2(g)} + O_{2(g)} ] × 6}\] |
| \[\ce{6CO_{2(g)} + 12H_{2(g)} -> C_6H_12O_{6(g)} + 6H_2O_{(l)}}\] |
|
\[\ce{6CO_{2(g)} + 12H_2O_{(l)} -> C_6H_12O_{6(g)} + 6H_2O_{(l)} + 6O_{2(g)}}\] |
It is more appropriate to write the reaction as given above because water molecules are also produced in the process of photosynthesis.
The path of this reaction can be investigated by using radioactive H2O18 in place of H2O.
RELATED QUESTIONS
Consider the reaction:
\[\ce{O3(g) + H2O2(l) → H2O(l) + 2O2(g)}\]
Why it is more appropriate to write these reaction as:
\[\ce{O3(g) + H2O2 (l) → H2O(l) + O2(g) + O2(g)}\]
Also, suggest a technique to investigate the path of the redox reactions.
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Balance the following equation in the basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent.
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\[\ce{H2C2O_{4(aq)} + MnO^-_{4(aq)}->CO2_{(g)} + Mn^2+_{( aq)}(acidic)}\]
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\[\ce{MnO^-_{4(aq)} + SO^{2-}_{3(aq)} -> MnO^{2-}_{4(aq)} + SO^{2-}_{4(aq)}}\]
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\[\ce{I2 + NO^{-}3 -> NO2 + IO^{-}3}\]
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\[\ce{I2 + S2O^{2-}3 -> I- + S4O^{2-}6}\]
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\[\ce{HgCl2 (aq) + 2KI (aq) -> HgI2 (s) + 2KCl (aq)}\]
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\[\ce{Cr2O^{2-}7 + Fe^{2+} + H+ -> Cr^{3+} + Fe^{3+} + H2O}\]
Balance the following ionic equations.
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\[\ce{xMnO^-_4 + yC2O^{2-}_4 + zH^+ -> xMn^{2+} + 2{y}CO2 + z/2H2O}\]
The values of x, y, and z in the reaction are, respectively:
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