Be sure to answer all parts. the first step in hno3 production is the catalyzed oxidation of nh3. without a catalyst, a different reaction predominates: 4 nh3(g) +3 o2 (g) ⇌ 2 n2(g) + 6 h2o(g) when 0.0150 mol of nh3(g) and 0.0150 mol of o2(g) are placed in a 1.00−l container at a certain temperature, the n2 concentration at equilibrium is 1.96 × 10−3 m. calculate kc.

The value of for the reaction is

Explanation:

We are given:

Initial moles of

Initial moles of

Volume of the container = 1.00 L

Molarity of the solution =

The given chemical equation follows:

Initial:          0.0150        0.0150

At eqllm:   0.0150-4x     0.0150-3x    2x       6x

The expression of for above equation follows:

        .......(1)

We are given:

Equilibrium concentration of

Equating the equilibrium concentrations of nitrogen, we get:

Calculating the equilibrium concentrations:

Concentration of

Concentration of

Concentration of

Concentration of

Putting values in expression 1, we get:

Hence, the value of for the reaction is

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the correct answer would be b. amelia, because the particals of gas move really fast (charged particals) and gas also has a lot of room (particals move independently) so the only answer that has both of those is amelia's.