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d1i1m1o1n [39]
3 years ago
15

Electron configuration of calcium

Chemistry
1 answer:
Eva8 [605]3 years ago
5 0
1s2 2s2 2p6 3s2 3p6 4s2 is the electron configuration for Calcium
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What is the molarity of a 3.0-liter solution that contains 0.45 moles of solute
sergeinik [125]
Moles = n/v where n is the moles of solute and v being the liters of solution.
We can put in the information provided to find the molarity.

Moles = .45/3.0 = .15
So we now know that the molarity of that solution is .15!
 I hope I helped you :). Make sure to memorize that formula because it's not that hard as long as you know what to plug in.
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What are the products for c3h8+o2-->co2+h2o
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Explanation:

3 0
2 years ago
A chemist prepares a solution of sodium thiosulfate (Na2S203) by measuring out 110.g of sodium thiosulfate into a 350. mL volume
forsale [732]

Answer:

1.99 M

Explanation:

The molar mass of sodium thiosulfate (solute) is 158.11 g/mol. The moles corresponding to 110 grams are:

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The molarity of sodium thiosulfate is:

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5 0
3 years ago
Upon dissolving in , undergoes a disproportionation reaction according to the following unbalanced equation: This disproportiona
pychu [463]

Answer:

The question in the narrative seems not to be complete because the unbalanced equation was not given and the values of the second(s) and  chemical dissolved was also not given.

Kindly find the complete question below and if you feel the question is still correct, the solution provided is still implies but without the values inserted.

Correct Question:

Upon dissolving InCl(s) in HCl , In(aq)  undergoes a disproportionation reaction according to the following unbalanced equation:

In ⁺ (aq) → In(s) → In³⁺ (aq)

This disproportionation follows first-order kinetics with a half-life of 667s. What is the concentration of In⁺ (aq) after 1.25 h if the initial solution of In⁺ (aq) was prepared by dissolving 2.38 g InCl(s) in dilute HCl to make 5.00 x 10² mL of solution? What mass of In(s) is formed after 1.25h?

Solution / Explanation:

Given half life of In⁺ at 66.7 s,

We recall the formula used in claculating the rate of constant for the first oreder reactin as :

K = 0.693 / t₁÷2,

Noting that:

t₁÷2 = half life

and K= rate constant

Therefore, if we replace the value of  t₁÷2  in the formular above,

We have,

K = 0.693 / 667s

K = 0.00 /s

Now, if we recall the mass of InCl(s) as 2.38g,

Volume of dilute HCl = 500 mL,

and the molar mass of  InCl(s) - 150.271 g/mol,

The number of moles is then calculated using the formular:

Number of moles: = Given Mass/Molar Mass

Now replacing the given values of given mass and the molar mass in the above formular,

= 2.38g / 150.271g/mol

= 0.0158 mol

Volume of diluted 500 mL.

Recalling also that we need to convert from mL into Liters

Therefore,  1mL = 10⁻³L

Therefore,

500mL = (500 X 10⁻³)L

0.5 L

Now, the molarrity of In⁺ (aq) is calculated using

morality of In⁺ (aq) = moles of In⁺ (aq)/volume of solution

= 0.0158/0.5L

=0.0316M (This is the initial concentration of In⁺ (aq))

The time of the reaction is 1.25h

There is 3600s in one hour

1.25h = 1.25 x 3600

= 4500s

7 0
3 years ago
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