a) What is the value of ∆H of the following chemical reaction? NaOH(aq) + HCl(aq) ----->...

a)

What is the value of ∆H of the following chemical reaction?

NaOH_(aq) + HCl_(aq) -----> NaCl_(aq) + H₂O_(l) + 55.216 kJ

b) Use the above equation to calculate the amount (in moles) of the water produced if you know that the mass of the solution was 100 g, the temperature change was 3^oC, and the specific heat of the solution is 4.184 J/^oC.g.

c) 54.6 kJ of heat is released when 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of NaCl and 1 mole of H₂O. Write a thermochemical equation for this reaction.

Expert Solution

NaOH_(aq) + HCl_(aq) -----> NaCl_(aq) + H₂O_(l) + 55.216 kJ

NaOH_(aq) + HCl_(aq) -----> NaCl_(aq) + H₂O_(l) H= - 55.216 kJ

b. q = mCT

= 100*4.184*30 = 12552J = 12.552KJ

from balanced equation

-55.216KJ enegy gives 1 moles of H2O

-12.552 KJ energy gives = 1*-12.552/-55.216 = 0.227moles of H2O

c. NaOH_(aq) + HCl_(aq) -----> NaCl_(aq) + H₂O_(l) H= - 54.6 kJ

queen_honey_blossom answered 6 months ago

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