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nignag [31]
9 months ago
6

water dissolves salts because it: select one: a. is hydrophobic, and salts are also hydrophobic. b. forms covalent bonds with th

e atoms of the salt crystal. c. has partial positive and negative charges. d. evaporates quickly at room temperature.
Chemistry
1 answer:
Gre4nikov [31]9 months ago
4 0

Salts get dissolved in water because it has partial positive and negative charges. So option (c) is correct.

<h3>Why does salt dissolves in water?</h3>

The water molecules pull the Na and Cl ions apart while breaking the ionic bond which held them together. After the salt ions are pulled apart, they get surrounded by water molecules. The salt dissolves to form a homogeneous solution.

  1. The slightly positive portion of sodium is attracted to the slightly negative portion of oxygen on the water molecule. At the same time, the slightly electronegative chlorine moieties of NaCl are attracted to the slightly electropositive hydrogen moieties of water.
  2. In either case, no true bond is formed, the stronger covalent bonds of water (also commonly held by hydrogen bonds between water molecules) win, NaCl gets pulled apart, resulting in dissociation of Na+ and Cl- ions with the Na+ and Cl- ions setting loosely in place between the intact H₂O molecules. NaCl is then ​dissolved​.

Salts are ionic and are expected to dissolve in water because water itself is polar. Therefore, ionic salts are expected to dissolve in polar solvents.

To know more about dissolution of salts in water visit:

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A certain first-order reaction has a rate constant of 2.15×10−2 s−1 at 20 ∘C. What is the value of k at 55 ∘C if Ea = 72.0 kJ/mo
adell [148]

Answer:

k_2=0.504s^{-1}

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the rate constant at 55 °C by using the temperature-variable version of the Arrhenius equation:

ln(\frac{k_2}{k_1} )=-\frac{Ea}{R}(\frac{1}{T_2} -\frac{1}{T_1} )

Thus, we plug in the temperatures, activation energy and universal constant of gases in consistent units to obtain:

ln(\frac{k_2}{0.0215s^{-1}} )=-\frac{72000\frac{J}{mol}}{8.3145\frac{J}{mol*K}}(\frac{1}{55+273} -\frac{1}{20+273} ) \\\\ln(\frac{k_2}{0.0215s^{-1}} )=3.154\\\\k_2=0.0215s^{-1}exp(3.154)\\\\k_2=0.504s^{-1}

Regards!

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stellarik [79]

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Describe melting of a solid
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3 years ago
What is the limiting reactant when 4 mol P4 and 4 mol S8 react.
In-s [12.5K]

Taking into account the reaction stoichiometry, P₄ will be the limiting reagent.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

8 P₄ + 3 S₈ → 8 P₄S₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

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<h3>Limiting reagent</h3>

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

<h3>Limiting reagent in this case</h3>

To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 3 moles of S₈ reacts with 8 moles of P₄, 4 moles of S₈ reacts with how many moles of P₄?

moles of P_{4} =\frac{4 moles of S_{8} x8 moles of P_{4} }{3 moles of S_{8}}

<u><em>moles of P₄= 10.667 moles</em></u>

But 10.667 moles of P₄ are not available, 4 moles are available. Since you have less amount of moles than you need to react with 4 moles of S₈, P₄ will be the limiting reagent.

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