Consider the following equilibrium: N204(8) = 2NO2(g) Suppose two different experiments were conducted on this equilibrium, at two different temperatures. Trial Temperature Initial Moles of N204 Equilibrium Moles of N204 1 25°C 1.00 0.815 2 55°C 1.00 0.500 What conclusion may be drawn from the above data? K> K, at all temperatures. The reaction is exothermic. The forward reaction proceeds faster than the reverse reaction. Kp = 1 at 55°C. The equilibrium constant increases with increasing temperature.

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Consider the following equilibrium:
N204(g) =
2NO2(g)
Suppose two different experiments were conducted on this equilibrium, at two
different temperatures.
Trial Temperature Initial Moles of N204 Equilibrium Moles of N204
1
25°C
1.00
0.815
55°C
1.00
0.500
What conclusion may be drawn from the above data?
O Kc> Kp at all temperatures.
The reaction is exothermic.
The forward reaction proceeds faster than the reverse reaction.
OKp =D1 at 55°C.
O The equilibrium constant increases with increasing temperature.
Transcribed Image Text:Consider the following equilibrium: N204(g) = 2NO2(g) Suppose two different experiments were conducted on this equilibrium, at two different temperatures. Trial Temperature Initial Moles of N204 Equilibrium Moles of N204 1 25°C 1.00 0.815 55°C 1.00 0.500 What conclusion may be drawn from the above data? O Kc> Kp at all temperatures. The reaction is exothermic. The forward reaction proceeds faster than the reverse reaction. OKp =D1 at 55°C. O The equilibrium constant increases with increasing temperature.
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