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3 years ago

[05.01] Which of the following best explains what happens when the kinetic energy of particles in a solid state increases?

2 answers:

3 0

The correct answer among the choices given is the third option. When the kinetic energy of particles on a solid state increases, the particles <span>vibrate fast enough to overcome the forces of attraction holding them together and become a liquid. This is due to the increase in the energy of motion in each particle.</span>

natali 33 [55]3 years ago

3 0

Answer:

They vibrate fast enough to overcome the forces of attraction holding them together and become a liquid.

Explanation:

Solids are more tightly packed than liquids. Liquids particles have a higher kinetic energy. When solid particles are heated, then the kinetic energy of the solid particle increases. Now the solid particles in their rigid structure show a greater vibrational motion.

Th higher vibrational motion helps the solid particles to overcome the intermolecular forces of attraction and thereby undergo a phase change forming liquids.

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Which laws can be combined to form the ideal gas law?

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Option 3- Avogadro's, Charles's and Boyle's

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2 years ago

If 507 g FeCl2 were used up in the reaction FeCl2 + 2NaOH Fe(OH)2(s) + 2NaCl, how many grams of NaCl would be made?

Ket [755]

Number of moles of FeCl2 used = mass/ molar mass
Number of moles = 507/126.751 = 4.
If one mole of Fe reacts with two moles of sodium
Then 4 moles of Fe produces 8 moles of sodium.
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3 years ago

Predict the sign of the entropy change,Delta S, for each of the following reactions:The signs are either going to be pos or nega

algol [13]

Answer: a) $Pb^{2+}(aq)+2Cl^-(aq)\rightarrow PbCl_2(s)$ : negative

b) $CaCO_3(s)\rightarrow CaO(s)+CO_2(g)$ : positive

c) $2NH_3(g)\rightarrow N_2(g)+3H_2(g)$ : positive.

d) $P_4(g)+5O_2(g)\rightarrow P_4O_{10}(s)$ : negative

e) $C_4H_8(g)+6O_2(g)\rightarrow 4CO_2(g)+4H_2O(g)$ : positive.

f) $I_2(s)\rightarrow I_2(g)$ : positive.

Explanation:

Entropy is the measure of randomness or disorder of a system. If a system moves from an ordered arrangement to a disordered arrangement, the entropy is said to decrease and vice versa.

$\Delta S$ is positive when randomness increases and $\Delta S$ is negative when randomness decreases.

a) $Pb^{2+}(aq)+2Cl^-(aq)\rightarrow PbCl_2(s)$

As ions are moving to solid form , randomness decreases and thus sign of $\Delta S$ is negative.

b) $CaCO_3(s)\rightarrow CaO(s)+CO_2(g)$

As solid is changing to gas, randomness increases and thus sign of $\Delta S$ is positive.

c) $2NH_3(g)\rightarrow N_2(g)+3H_2(g)$

As 2 moles of reactants are converted to 4 moles of products , randomness increases and thus sign of $\Delta S$ is positive.

d) $P_4(g)+5O_2(g)\rightarrow P_4O_{10}(s)$

As gas is changing to solid, randomness decreases and thus sign of $\Delta S$ is negative.

e) $C_4H_8(g)+6O_2(g)\rightarrow 4CO_2(g)+4H_2O(g)$

As 7 moles of reactants are converted to 8 moles of products , randomness increases and thus sign of $\Delta S$ is positive.

f) $I_2(s)\rightarrow I_2(g)$

As solid is changing to gas, randomness increases and thus sign of $\Delta S$ is positive.

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3 years ago

Which of the following reasons is why spent fuel rods are stored in a pool of water?

lukranit [14]

Answer:

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2 years ago