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Question
The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows.
N2(g) + 3 H2(g) 
2 NH3(g) DH = -92.2 kJ
Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the left?
A.adding N2(g)
B.removing NH3(g)
C.adding a catalyst
D.decreasing the temperature
E.removing H2(g)
Answer
This answer is hidden. It contains 2 characters.
Related questions
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Q:
Assume that the following endothermic chemical reaction is at equilibrium.
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2/ Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g).
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Q:
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B.
C.
D.
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Q:
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Q:
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Q:
Hydrogen peroxide decomposes into water and oxygen in a first-order process.
H2O2(aq) H2O() + 1/2 O2(g)
At 20.0 C, the half-life for the reaction is 3.92 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 7.00 days?
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Q:
A student analyzed a first-order reaction and obtained the graph below. Unfortunately, the student forgot to label the axes. What are the correct labels for the x and y axes? A.x axis = time, y axis = ln[A]
B.x axis = ln[time], y axis = [A]
C.x axis = ln[time], y axis = [A]
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E.x axis = 1/time, y axis = 1/[A]
Q:
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