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Answer the questions by looking at the following reaction between nitrogen oxides.

N2O(g) + NO2(g) → 3NO(g)
(a) Find the values ​​of ΔH°, ΔS°, ΔG°
(b) Assuming that ΔH° and ΔS° do not change with temperature, calculate ΔG° at 800 K. 800 K, is this reaction spontaneous under standard conditions?
(c) Calculate ΔG° at 1000 K. Is this reaction spontaneous at this temperature and at standard conditions?

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  1. I suppose I don't understand why you're having trouble unless you're looking for someone to do all of the work.
    a. Look up the values in a table. If you don't have a table look them up on the web.
    b. dG = dH - TdS. Plug in the values from a. The reaction is spontaneous @ 800 K if dG is negative.
    c. Change 800 K to 1000 K and recalculate b.
    Post your wor if you get stuck but include the values you found in part a and your calculations for b and c..

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