Time Consider the reaction represented by the equation 2X + 22 - X,Z,. During a reaction in which a large excess of reactant X was present, the concentration of reactant Z was monitored over time. A plot of the natural logarithm of the concentration of Z versus time is shown in the figure above. The order of the reaction with respect to reactant Z is Izl uI

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Time
Consider the reaction represented by the equation
2 X + 2Z X,Z2. During a reaction in which
a large excess of reactant X was present, the
concentration of reactant Z was monitored over
time. A plot of the natural logarithm of the
concentration of Z versus time is shown in the
figure above. The order of the reaction with
respect to reactant Z is
(A) zero order
(B) first order
(C) second order
(D) third order
Transcribed Image Text:Time Consider the reaction represented by the equation 2 X + 2Z X,Z2. During a reaction in which a large excess of reactant X was present, the concentration of reactant Z was monitored over time. A plot of the natural logarithm of the concentration of Z versus time is shown in the figure above. The order of the reaction with respect to reactant Z is (A) zero order (B) first order (C) second order (D) third order
N2(8) + 3 H,(g) 2 2 NH,(8)
AH398 =-92 kJ/mol,i AG298 =-33 kJ/mol,
Consider the reaction represented above at 298 K.
When equal volumes of N,(g) and H,(g), each at
1 atm, are mixed in a closed container at 298 K,
no formation of NH,(g) is observed. Which of the
following best explains the observation?
(A) The N2(g) and the H,(g) must be mixed in a
1:3 ratio for a reaction to occur.
(B) A high activation energy makes the forward
reaction extremely slow at 298 K.
(C) The reaction has an extremely small
equilibrium constant, thus almost no
product will form.
(D) The reverse reaction has a lower activation
energy than the forward reaction, so the
forward reaction does not occur.
Transcribed Image Text:N2(8) + 3 H,(g) 2 2 NH,(8) AH398 =-92 kJ/mol,i AG298 =-33 kJ/mol, Consider the reaction represented above at 298 K. When equal volumes of N,(g) and H,(g), each at 1 atm, are mixed in a closed container at 298 K, no formation of NH,(g) is observed. Which of the following best explains the observation? (A) The N2(g) and the H,(g) must be mixed in a 1:3 ratio for a reaction to occur. (B) A high activation energy makes the forward reaction extremely slow at 298 K. (C) The reaction has an extremely small equilibrium constant, thus almost no product will form. (D) The reverse reaction has a lower activation energy than the forward reaction, so the forward reaction does not occur.
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