Chemistry, 30.03.2021 01:00 iibabycarrotsii

Consider the reaction below. H O single bonded to C double bonded above to O and to the right to the bottom left of a benzene ring. The ring is bonded from the upper right to a C double bonded above to O and to the right to O H. H O bonded to C H Subscript 2 Baseline C H Subscript 2 Baseline bonded to O H. Arrow pointing with bond H Subscript 2 Baseline O beside it pointing down to H O bonded to C double bonded above to O and to the right to the bottom left of a benzene ring. The ring is bonded from the upper right to a C double bonded above to O and to the right to O bonded to C H Subscript 2 Baseline C H Subscript 2 Baseline bonded to O H.
This reaction eventually forms this product.

A bond from left to O single bonded to C double bonded above to O and to the right to the bottom left of a benzene ring. The ring is bonded from the upper right to a C double bonded above to O and to the right to O bonded to C H Subscript 2 Baseline C H Subscript 2 Baseline bonded to O bonded to C double bonded above to O and right to the upper left corner of a benzene ring. The ring is bonded from the lower left to C double bonded above to O and single bonded right to O bonded to CH Subscript 2 Baseline C H Subscript 2 Baseline bonded right to O bonded to C double bonded above to O and right to the lower left of a benzene ring, which is bonded from upper right to C double bonded above to O and single bonded right to O bonded to C H Subscript 2 Baseline C H Subscript 2 Baseline bonded to O.
Which type of reaction is represented by these diagrams?

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Answer from: Quest

the balanced equation for reaction of ca metal with o2 to produce cao is as below

2 ca+ o2→ 2 cao2

explanation

the reaction is balanced since the number of atoms in reactant side is equal to number of atoms in product side. for example they are 2 atom of ca in reactant side and 2 atoms of ca in the product side.

the process is a meet the requirement of redox reaction because : calcium is oxidized from oxidation state 0 to 2+ while oxygen is reduced from oxidation state 0 to 2-

Answer from: Quest

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.

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answer:

technetium is the most reactive. this is followed by silver. the least reactive out of these three elements is strontium.

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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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Consider the reaction below. H O single bonded to C double bonded above to O and to the right to th...

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