Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless ... At High Temperature the red color is strong ... At Low Temperature the gas has less color ... If we represent the equilibrium as: ... 2 NO2 (g) Doublearrow. GIFN2O4 (g) We can conclude that:1. This reaction is:A. ExothermicB. EndothermicC. NeutralD. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of NO2:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.

Question

Kylan Padilla

Chemistry

30 January, 04:05

Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless ... At High Temperature the red color is strong ... At Low Temperature the gas has less color ... If we represent the equilibrium as: ... 2 NO2 (g) Doublearrow. GIFN2O4 (g) We can conclude that:1. This reaction is:A. ExothermicB. EndothermicC. NeutralD. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of NO2:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.

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Answers (1)

Know the Answer?

Scarlett Stafford · Answer 1

1-C

2-A

3-B

Explanation:

K=[N204]/[NO2]

In the first question the reaction is at equilibrium. When the temperature is decreased, more N2O4 if formed and K increases. When the temperature is increased, more NO2 is formed and K decreases.