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saveliy_v [14]
4 years ago
3

Compare the modern (electron cloud) model of the atom with Dalton’s atomic model. Which of these statements describe the two mod

els correctly? Check all of the boxes that apply. Dalton’s model was replaced only because of its age. Dalton’s model represented atoms as indivisible, but the modern theory recognizes that they contain smaller particles. The modern model explains all available data about atoms; Dalton’s model does not. The modern model is more widely accepted because it was proposed by more well known scientists.
Chemistry
2 answers:
GrogVix [38]4 years ago
6 0

Dalton’s model represented atoms as indivisible, but the modern theory recognizes that they contain smaller particles.

The modern model explains all available data about atoms; Dalton’s model does not.

Mama L [17]4 years ago
3 0
The correct answer for this question is this one:

<span>- The modern model explains all available data about atoms; Dalton’s model does not.
- </span>Dalton’s model represented atoms as indivisible, but the modern theory recognizes that they contain smaller particles
Hope this helps answer your question and have a nice day ahead.
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There is no diagram attached but there are some ways by which you can find it too easily by yourself

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Strong acids are those that ionizes almost completely in water. to be considered a strong acid, an acid must have an acid ioniza
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Ka  is  the  equilibrium  constant  for  the  ionization for a reaction. It  is  calculated  as  follows
ka  is equal  to (H3o ions)(A-) divided by (HA)
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What is the number of each element and the total number of atoms for vinegar?
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4 0
3 years ago
Suppose 0.245 g of sodium chloride is dissolved in 50. mL of a 18.0 m M aqueous solution of silver nitrate.
Bezzdna [24]

Answer:

\large \boxed{\text{ 0.066 mol/L}}

Explanation:

We are given the amounts of two reactants, so this is a limiting reactant problem.

1. Assemble all the data in one place, with molar masses above the formulas and other information below them.

Mᵣ:       58.44  

            NaCl + AgNO₃ ⟶ NaNO₃ + AgCl

m/g:     0.245

V/mL:                 50.

c/mmol·mL⁻¹:       0.0180

2. Calculate the moles of each reactant  

\text{Moles of NaCl} = \text{245 mg NaCl} \times \dfrac{\text{1 mmol NaCl}}{\text{58.44 mg NaCl}} = \text{4.192 mmol NaCl}\\\\\text{ Moles of AgNO}_{3}= \text{50. mL AgNO}_{3} \times \dfrac{\text{0.0180 mmol AgNO}_{3}}{\text{1 mL AgNO}_{3}} = \text{0.900 mmol AgNO}_{3}

3. Identify the limiting reactant  

Calculate the moles of AgCl we can obtain from each reactant.

From NaCl:  

The molar ratio of NaCl to AgCl is 1:1.

\text{Moles of AgCl} = \text{4.192 mmol NaCl} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol NaCl}} = \text{4.192 mmol AgCl}

From AgNO₃:  

The molar ratio of AgNO₃ to AgCl is 1:1.  

\text{Moles of AgCl} = \text{0.900 mmol AgNO}_{3} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol AgNO}_{3}} = \text{0.900 mmol AgCl}

AgNO₃ is the limiting reactant because it gives the smaller amount of AgCl.

4. Calculate the moles of excess reactant

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 I/mmol:      0.900        4.192            0

C/mmol:    -0.900       -0.900        +0.900

E/mmol:      0                3.292          0.900

So, we end up with 50. mL of a solution containing 3.292 mmol of Cl⁻.

5. Calculate the concentration of Cl⁻

\text{[Cl$^{-}$] } = \dfrac{\text{3.292 mmol}}{\text{50. mL}} = \textbf{0.066 mol/L}\\\text{The concentration of chloride ion is $\large \boxed{\textbf{0.066 mol/L}}$}

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Hope this helps! :)

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