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Question
Which of the following statements is true concerning the reaction below?
CH4(g) + N2(g) → HCN(g) + NH3(g); 
Hº= 164.1kJ; Gº= 159.1kJ at 298K
A) It is nonspontaneous at all temperatures.
B) It is spontaneous at relatively low temperatures only.
C) It is spontaneous at all temperatures.
D) It is at equilibrium at 298 K.
E) It is spontaneous at relatively high temperatures only.
Answer
This answer is hidden. It contains 1 characters.
Related questions
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Q:
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Q:
If the Thomson model of the atom had been correct, Rutherford would have observed
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Q:
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B) CO(g) + H2O(g) CO2(g) + H2(g)
C) CO(g) + 3H2(g) CH4(g) + H2O(g)
D) CaO(s) + CO2(g) CaCO3(s)
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Q:
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Q:
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Q:
Which of the following represents a dynamic equilibrium?
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Q:
For the hypothetical reaction A → products, the concentration of A was monitored over time. From the following graph, what is the rate constant for the decomposition of A?A) -0.02735 s-1B) 2.3026 s-1C) -2.3026 s-1D) 0.02735 s-1E) 0.01188 s-1
Q:
Which of the following corresponds to the correct equation for the half-life of a first-order reaction?A) B) C) D) E)
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Q:
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Q:
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Q:
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Q:
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Q:
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Q:
If a reaction is first-order with respect to a particular reactant, when the concentration of that reactant is increased by a factor of 2, the reaction rate will _____.
A) increase by a factor of 2.
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C) decrease by a factor of .
D) decrease by a factor of .
E) increase by a factor of 4.
Q:
For a certain first-order reaction with the general form aA → products, the rate is 0.32 M·s-1 when the concentration of the reactant is 0.29M. What is the rate constant for this reaction?A) 0.26 s-1B) 1.1 s-1C) 0.32 s-1D) 3.1 s-1E) 3.8 s-1