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lisabon 2012 [21]
3 years ago
7

how many moles of hydrogen are evolved when an excess of sodium metal is added to one mole of citric acid?

Chemistry
1 answer:
vova2212 [387]3 years ago
4 0
The formula of citric acid is:

           CO2H
           |
HO -  C - CH2CO2H
          
|
          C - CH2 CO2H



I bolded the 4 hydrogens that can be subsituted by sodium.


Three of those hydrogens belong to carboxyl group (- CO2H) and one to a hydroxyl group (- OH).


You need to take into account that 4 H will form 2 H2 molecules.


So, the answer is that 2 moles of molecules will be formed from 1 mole of citric acid molecules.


   

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According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

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(1) B_2O_3(s)+3H_2O(g)\rightarrow 3O_2(g)+B_2H_6(g)     \Delta H_A=+2035kJ

(2) 2B(s)+3H_2(g)\rightarrow B_2H_6(g)    \Delta H_B=+36kJ

(3) H_2(g)+\frac{1}{2}O_2(g)\rightarrow H_2O(l)    \Delta H_C=-285kJ

(4) H_2O(l)\rightarrow H_2O(g)    \Delta H_D=+44kJ

Now we have to revere the reactions 1 and multiple by 2, revere the reactions 3, 4 and multiple by 2 and multiply the reaction 2 by 2 and then adding all the equations, we get :

(when we are reversing the reaction then the sign of the enthalpy change will be change.)

The expression for enthalpy of the reaction will be,

\Delta H=-2\times \Delta H_A+2\times \Delta H_B-6\times \Delta H_C-6\times \Delta H_D

\Delta H=-2(+2035kJ)+2(+36kJ)-6(-285kJ)-6(+44)

\Delta H=-2552kJ

Therefore, the enthalpy of the reaction is, -2552 kJ/mole

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