Question 1 Calculate the change in H for the reaction 2N2(g) + O2(g) + 3H2(g) - 2NO(g) + 2NH3(g), from the following data.
N2 (g) + O2 (g) – 2 NO (g) H = -180.5 kJ
N2 (g) + 3 H2 (g) - 2 NH3(g) H=-91.8 kJ
Your
-16.7 K)
-272.3K
-544.6 ki

gas

explanation:

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Electrical charges of ionic bonds

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.