a. Write the net equations for : HCl (aq) + NaOH(aq) HCl (aq) +NaOH (s) HCl(aq)+

Question

a. Write the net equations for :

HCl (aq) + NaOH(aq)

HCl (aq) +NaOH (s)

HCl(aq)+NaOH(aq)

b. what is the relationship among the chemical equations? can any two be combined to form the third?

c. are the reactions exothermic or endothermic? if an exothermic reaction is reversed, will it be exothermic or endothermic? explain why

d.which reaction had the highest averge heat per mole rxn? which had the smallest and the middle?

e. how do the relationships among the chemical equations in part b compare with the relationships among the heats of reaction?

f. draw a particle view of these three reactions showing the relationship between their equations and heats of reaction in KJ/ mol

Thank you!!!!

Explanation / Answer

1..H2o(aq) + NaOH(s) = NaCl(aq) + H2O(l)

2...HCl(aq) + NaOH(s) = NaCl(aq) + H2O(l)

3..HCl(aq) + NaOH(aq) = NaCl(aq) + H2O(l)

Double replacement reaction ( neutralizing reaction)

B..not to combined each other

C...exothermic reaction released heat and mix solution cool.

While revert is endothermic because NaCl require energy for dissolving.

D....H2o(aq) + NaOH(s) = NaCl(aq) + H2O(l) has higher heat energy per mole..because solid NaOH have hygroscopic nature...

e...Chemical Reaction: NaOH(s) + HCl(aq) NaCl(aq) + H2O(l)
Heat of formation:.....-425.93 .... -92.30 ...... -407.27 ... -285.83 ... all in kJ/mol

Hess's Law: H(rxn) = Sum[H(f) products] - Sum[H(f) reactants]

H(rxn) = [(1 mol)(-407.27 kJ/mol) + (1 mol)(-285.83 kJ/mol)] - [(1 mol)(-425.93 kJ/mol) + (1 mol)(-92.30)

F...[1Hf(H2O ()) + 1Hf(NaCl (aq))] - [1Hf(HCl (aq)) + 1Hf(NaOH (aq))]
[1(-285.83) + 1(-407.25)] - [1(-167.15) + 1(-470.09)] = -55.8399999999999 kJ
-55.84 kJ     (exothermic)

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