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One mole of Al4C3(s) reacts with H2O in a closed vessel at 27°C against atmospheric pressure. Work done (in cal) is....?
Correct answer is '0'. Can you explain this answer?
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One mole of Al4C3(s) reacts with H2O in a closed vessel at 27°C ag...
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Aluminum carbide reacts with water to form aluminium hydroxide and methane gas.
Reaction can be represented as follows -
Al4C3(s) + 12H2O(l) → 4Al(OH)3(aq) + 3CH4(g)
Ideal gas equation takes only gaseous products into consideration, thus ∆n = 3 .
Work done during the process -
W = - ∆n � R � T
W = - 3 � 8.314 � 300
W = -7482 J
W = -7.482 kJ
Work done during the reaction is -7.482 kJ.
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One mole of Al4C3(s) reacts with H2O in a closed vessel at 27°C ag...
The balanced chemical equation for the reaction between Al4C3 and H2O is:
Al4C3 + 12 H2O -> 4 Al(OH)3 + 3 CH4
From the balanced equation, we can see that for every mole of Al4C3, 12 moles of H2O are required to fully react.
Given that we have one mole of Al4C3, we need 12 moles of H2O to react completely.
The reaction takes place in a closed vessel, which means the volume of the reactants and products will remain constant.
Therefore, the volume of H2O required to react with one mole of Al4C3 in a closed vessel at 27°C cannot be determined based on the information given.
Al4C3 + 12 H2O -> 4 Al(OH)3 + 3 CH4
From the balanced equation, we can see that for every mole of Al4C3, 12 moles of H2O are required to fully react.
Given that we have one mole of Al4C3, we need 12 moles of H2O to react completely.
The reaction takes place in a closed vessel, which means the volume of the reactants and products will remain constant.
Therefore, the volume of H2O required to react with one mole of Al4C3 in a closed vessel at 27°C cannot be determined based on the information given.
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One mole of Al4C3(s) reacts with H2O in a closed vessel at 27°C against atmospheric pressure. Work done (in cal) is....?Correct answer is '0'. Can you explain this answer?
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