Chemistry, 14.11.2019 03:31 bennettaly2452

The reaction between carbon tetrachloride, ccl4, and water, h2o, to form carbon dioxide, co2, and hydrogen chloride, hcl, has a ? g? value of ? 232 kj/mole, and so is thermodynamically favored. but when you mix carbon tetrachloride with water, no change is observed. what is a possible explanation for this? a)it is a slow reaction kinetically. b)the activation energy of the reaction is too small. c)the reaction is not spontaneous. d)the reaction is not favored thermodynamically

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Answer from: thebiggestbigbilly

a)It is a slow reaction kinetically.

Explanation:

The reaction of CCl₄ with H₂O is:

CCl₄ + H₂O → CO₂ + HCl the ΔG is -232kJ/mol

As ΔG<0 the reaction is spontaneous, that means the reaction is themodynicamically favored. Thus, c and d are false.

The activation energy is defined as the minimum amount of energy that is required for a reaction occurs, if the activation energy of the reaction is small, will be easy that the reaction occurs, thus, b is false.

In a chemical reaction, there are involve the thermodynamic and kinetic items. The reaction is thermodynamically favored but there is no data about kinetics of the reaction. Thus it is possible that is a slow reaction doing a true.

I hope it helps!

Answer from: Quest

i believe it is c.) 1575 j.

Answer from: Quest

Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbf₂(s) ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is $k_{sp} = [\text{pb}^{2+}][\text{f}^- ]^2 = 4 \times 10^{-8}$ (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as $q = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}}$ 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: $\begin{aligned} q & = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}} \\ & = (1.9 \times 10^{-3} ) (3.8\times 10^{3})^2 \\ & = 2.7 \times 10^{-8} \end{aligned}$ since q = 2.7 × 10⁻⁸ < ksp = 4 × 10⁻⁸, a precipitate will not form.

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The reaction between carbon tetrachloride, ccl4, and water, h2o, to form carbon dioxide, co2, and hy...