This quiz, titled 'Chapter 18 Reaction Rates and Equilibrium Part 2', dated 3\/13\/11, explores key concepts in thermodynamics, such as entropy changes and spontaneity in chemical reactions. It assesses understanding of how entropy and enthalpy determine reaction spontaneity, crucial for advanced chemistry studies.
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The size and direction of heat (enthalpy) changes and entropy changes together determine whether a reaction is spontaneous.
The size and direction of moisture(enthalpy) changes and entropy changes together determine whether a reaction is spontaneous.
The size and amount of heat (enthalpy) changes and entropy changes together determine whether a reaction is spontaneous.
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Because both factors are favorable too many
Because both factors are not favorable
Because both factors are favorable
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Not favored
Favored
Small
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J; P/S
R; J/P
S; J/K
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S exponent 0
S exponent 9
S exponent 4
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101.9 kPa
101.3 kPa
101.6 kPa
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-0
4
0
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ΔS0 =S exponent 1 (products) - S exponent -1 (reactants)
ΔS0 =S exponent 0 (products) - S exponent -0 (reactants)
ΔS0 =S exponent 0 (products) - S exponent 0 (reactants)
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98.7 J/Kmol
88.7 J/Kmol
108.7 J/Kmol
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Work
Rest
Product
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ΔG = ΔH =TΔS, where ΔH is the change in enthalpy, ΔS is the change in entropy, and temperature (T) is in kelvins.
ΔG = ΔH =TΔS, where ΔH is the no change in enthalpy, ΔS is the change in entropy, and temperature (T) is in kelvins.
ΔG = ΔH =TΔS, where ΔH is the small change in enthalpy, ΔS is the change in entropy, and temperature (T) is in kelvins.
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Negative, positive
Positive, negative
Both negative, positive and positive, negative
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ΔGexponent0 = ΔH exponent 0=TΔS0, where ΔH exponent 0 and ΔS exponent 0 are known, and the temperature (T) is in kelvins.
ΔG exponent 0 = ΔHexponent0=TΔSexponent 0, where ΔHexponent 0 and ΔSexponent 0 are unknown, and the temperature (T) is in kelvins.
ΔG exponent 0 = ΔH exponent 0=TΔS exponent 0, where ΔH exponent 0 and ΔS exponent 0 are known, and the temperature (T) is in kelvins.
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You use ΔG exponent 0 f , the standard free-energy change for the formation of substances from their elements. The formula is ΔG0 = ΔG exponet 0 f (products) = ΔG exponent0 f (reactants).
You use ΔG exponent 0 f , the standard free-energy no change for the formation of substances from their elements. The formula is ΔG0 = ΔG exponet 0 f (products) = ΔG exponent0 f (reactants).
You use ΔG exponent 0 t , the standard free-energy no change for the formation of substances from their elements. The formula is ΔG0 = ΔG exponet 0 f (products) = ΔG exponent0 f (reactants).
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It is a reaction with ore than one activated complex between the reactants and the products.
It is a reaction with only one activated complex between the reactants and the products.
It is a reaction with only one activated complex between the reactants and the heat.
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The constant is a proportionality constant relating the concentrations of chemical change to the rate of the reaction.
The constant is a proportionality constant relating the concentrations of reactants to the rate of the reaction.
The constant is a proportionality constant relating the concentrations of product to the rate of the reaction.
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Product
Amount
Order
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Two or more reactants
Both reactants and products
Only one reactant
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The actual chemical order must be determined by experiment.
The actual kinetic order must be determined by experiment.
The actual potential order must be determined by experiment.
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A reaction progress curve is a graph of all the energy changes that occur as reactants are converted to products.
A reaction progress curve is a graph of all the energy changes that occur as products are converted to reactants.
A reaction progress curve is a graph of all the energy changes that occur as kentic energy is converted to products.
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Major
Elementary
Median
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It is a product of a reaction that becomes a reactant of same reaction.
It is a reaction of a product that becomes a reactant of another reaction.
It is a product of a reaction that becomes a reactant of another reaction.
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