A 1.3 g sample of a substance is heated from 0°C to 45°C and is found to have absorbed 45 j of heat. What is the specific heat o
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Answer:
I. Kindly, see the attached image.
II. The reaction is exothermic.
III. - 51.88 kJ/mol.
IV. The reaction is spontaneous.
Explanation:
I. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction.
- Since the sign of ΔH is negative, the reaction is exothermic reaction.
In an exothermic reaction, the energy of the reactants is higher than that of the products.
<u><em>Kindly see the attached image to show you the potential energy diagram of the reaction.</em></u>
<em>II. Is the reaction endothermic or exothermic? Explain your answer.</em>
- The reaction is exothermic reaction.
- The sign of ΔH indicates wither the reaction is endothermic or exothermic one:
If the sign is positive, the reaction is endothermic.
If the sign is negative, the reaction is exothermic.
Herein, <em>ΔH = - 33.1 kJ/mol, </em>so the reaction is exothermic.
<em>III. What is the Gibbs free energy of the reaction at 25°C? </em>
∵ ΔG = ΔH - TΔS.
Where, ΔG is the Gibbs free energy change (J/mol).
ΔH is the enthalpy change (ΔH = - 33.1 kJ/mol).
T is the temperature (T = 25°C + 273 = 298 K).
ΔS is the entorpy change (ΔS = 63.02 J/mol.K = 0.06302 J/mol.K).
<em>∴ ΔG = ΔH - TΔS</em> = (- 33.1 kJ/mol) - (298 K)(0.06302 J/mol.K) = <em>- 51.88 kJ/mol.</em>
IV. Is the reaction spontaneous or nonspontaneous at 25°C?
The sign of ΔG indicates the spontaneity of the reaction:
If ΔG < 0, the reaction is spontaneous.
If ΔG = 0, the reaction is at equilibrium.
If ΔG > 0, the reaction is nonspontaneous.
Herein, <em>ΔG = - 51.88 kJ/mol, </em>so the reaction is spontaneous.
