Which of the following scenarios below best describes how to verify Hess’s Law (1 mark) (I:1)单项选择题

A

a. Measure the change in temperature of a reaction at different concentrations and compare it with the temperature change of a reaction at constant concentration.

B

b. Measure the enthalpy change of a reaction in a single step and compare it with the sum of the enthalpy changes of multiple reactions that combine to give the same overall reaction.

C

c. Calculate the equilibrium constant for a reaction and compare it with the equilibrium constants of reactions that are combined to give the same overall reaction.

D

d. Determine the reaction rate of a given reaction and compare it with the rate of a different reaction that produces the same products.

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类似问题

Question textAspirin (C9H8O4) is susceptible to degradation by hydrolysis if exposed to water, forming salicylic acid (C7H6O3) and acetic acid (CH3COOH): C9H8O4 (s) + H2O (l) → C7H6O3 (s) + CH3COOH (l) Given the following enthalpies of formation, calculate the enthalpy of the above hydrolysis process per mole of aspirin. State whether the hydrolysis is endothermic or exothermic, justifying your choice from the options available. ∆H°f[C9H8O4 (s)] = −736.4 kJ mol-1 ∆H°f[H2O (l)] = −285.8 kJ mol-1 ∆H°f[C7H6O3 (s)] = −588.4 kJ mol-1 ∆H°f[CH3COOH (l)] = −484.1 kJ mol-1 The enthalpy of hydrolysis is Answer 1 Question 9[input] kJ mol-1 and the hydrolysis is Answer 2 Question 9[select: , exothermic, endothermic] because Answer 3 Question 9[select: , the total number of moles of gas does not change, heat is absorbed from the surroundings during the formation of each of the reactants and products, heat is released to the surroundings during the formation of each of the reactants and products, the system absorbs heat from the surroundings during the hydrolysis, the system releases heat to the surroundings during the hydrolysis, the entropy change during the hydrolysis is negligible]

Determine the unknown reaction enthalpy change using the enthalpy changes provided, input your numerical answer (numbers only) below in kJ mol-1: A (l) + D (l) + H (l) → J (s) + M (g) ΔH°rxn = ? A (l) + H (l) → Z (l) ΔH°1 = -12.3 kJ mol-1 J (l) + M (g) → Z (l) + D (l) ΔH°2 = 44.5 kJ mol-1 J (s) → J (l) ΔH°3 = 8.77 kJ mol-1

Consider the following thermochemical equations:C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) ΔH = - 1,323 kJ mol-1 H2O(l) →  H2O(g) ΔH = + 44 kJ mol-1Determine the value of the enthalpy change for the following reaction: C2H4(g) + 3O2(g) →  2CO2(g) + 2H2O(l) ΔH = ?

Consider the accompanying chemical equation:2SO2(g) + O2(g) →  2SO3(g) Find the heat of reaction for this equation given the following two heats of formation:Enthalpy of formation of SO2(g) = -296.8 kJ / mole Enthalpy of formation of SO3(g) = -395.7 kJ / mole

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