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Exam 12: Spontaneity of Chemical Processes

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Question 1

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Complete the following table for determining at what relative temperature (high or low, or at none) a reaction will be spontaneous.

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Question 2

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Given three identical cups and three identical marbles, which of the following arrangements has the greatest value of W?

A) one marble in each cup
B) two marbles in one cup, one marble in one of the other cups
C) all three marbles in one cup
D) all have the same values of W
E) two of them have the same value of W

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Question 3

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At what identical concentration of H⁺ and CH₃CO₂^- (?G°_f = -372.5 kJ) will the dissociation of 1 M acetic acid, below, ( $\Delta$ G°_f (CH₃CO₂H (aq)) = -399.6 kJ) become spontaneous at room temperature? CH₃CO₂H (aq) $\rightarrow$ H⁺(aq) + CH₃CO₂^-(aq)

Calcite, CaCO_3(s), can be converted to CaO_(s) and CO_2(g). Determine the pressure of CO₂ at 1150 K at which the reaction is no longer spontaneous.

What is the entropy change for the reaction of graphite (S˚=5.74 J/mol•K) and hydrogen (S˚=130.68) to produce methane (S˚=186.2)?

Consider the following unbalanced reaction:CO₂(g) + H₂O(g) (\rarr\) O₂(g) + C₃H₈(g) This reaction is endothermic.

What is the entropy change in the surroundings when the system is a 2.2 kg block of ice that melts in a swimming pool (surrounding) whose temperature is 31°C?

Recognize the driving force behind all chemical change: dispersal of energy and matter.

Palmitic acid, C₁₅H₃₁CO₂H undergoes complete combustion with $\Delta$ G_rxn ^o of -9790 kJ mol^-1. Using bond energies, estimate the entropy change associated with this reaction.

Which of the following arrangements of 4 identical socks in a 4-drawer dresser has the least degree of disorder?

The standard molar entropy of NO is 211 J K^-1 mol^-1. What is the standard entropy of 3 moles of NO at 10 bar?

In adjusting the acidity of swimming pool water, concentrated aqueous HCl is added. What is the entropy for the chloride ions after 0.5 L of 12.0 M HCl is added to a swimming pool of 9.6 x 10⁴ L (about 25,000 gallons)? (S° Cl^- _(aq) = 56.5 J/mole • K)

Determine Gibb's Free Energy and if the following unbalanced reaction is spontaneous at 0^oC. Ba(OH)₂.8H₂O_(s) + NH₄NO_3(s) $\rarr$ Ba(NO₃)_2(s) + H₂O_(l) + NH_3(aq)

Considerable energy is required to vapourize water, yet water does evaporate as demonstrated by clothes drying when hung out. The reason for this spontaneous process is

How does your body perform non-spontaneous reactions?

An explosive that is also used as fertilizer is ammonium nitrate. Calculate $\Delta$ G $\degree$ for one of the decomposition reactions this fertilizer can undergo. ( $\Delta$ G $\degree$ = -183.9 (NH₄NO₃), 103.7 (N₂O), -228.7 (H₂O) in kJ/mol) NH₄NO_3(s) $\rightarrow$ N₂O_(g) + 2 H₂O_(g)

The exothermic oxychlorination of ethylene to vinyl chloride is shown below:CH₂CH_2(g) + HCl_(g) + $\frac{1}{2}$ O_2(g) $\rarr$ CH₂CHCl_(g) + H₂O_(g) What are the signs for the entropy change of the system and surroundings, respectively?

Glucose (MM = 180g/mole) is metabolized at a rate of about 38% efficiency. How many grams of glucose would supply the energy to ride a bicycle at 35 km/hour for 1 hour, an activity that would require about 1500 kJ of energy?

Calculate the free energy for the oxychlorination of ethylene to vinyl chloride, CH₂CHCl, under standard conditions at 100^oC given the thermodynamic data below collected at 25^oC: $\Delta$ G^o = 53.6(CH₂CHCl), -95.3(HCl), 68.49(CH₂CH₂), -228.7(H₂O) kJ/mol $\Delta$ H^o = 37.2(CH₂CHCl), -92.3(HCl), 52.4(CH₂CH₂), -241.8(H₂O) kJ/molThe equation of reaction is: CH₂CH_{2 (g)} + HCl _(g) + $\frac{1} {2}$ O_{2 (g)} $\rarr$ CH₂CHCl _(g) + H₂O _(g)

The conversion of calcite,CaCO_3(s), to CaO_(s) and CO_2(g) is NOT favourable at ambient temperatures. At what temperature will this decomposition of CaCO₃ become spontaneous?