A student is shown a simple model of particles that make up a liquid, as shown su
How should the model be changed to show the particles of a liquid at a higher temperature?
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A. Separate the particles into positive and negative charges, and increase the space between the particles
B. Separate the particles into positive and negative charges, but maintain the same space between the particles
C Decrease the velocities of the particles, and decrease the space between the particles.
D. Increase the velocities of the particles, but maintain the same space between the particles.

The answer is b i think

Iimpact me by the one the yet but him.

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.

The answer would be true