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NeTakaya
3 years ago
11

Calculate the heat required to convert 5.0 g of ice at 0.0 c to steam at 100

Chemistry
1 answer:
Fiesta28 [93]3 years ago
6 0
Heat= latent heat of fusion+sensible heat+ latent heat of vapourization
=(79.7*5)+(5*100*1)+(540*5)
=3598.5 cal
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How many atoms are in 3.5 moles of He?
Volgvan

Answer:

The answer is 2.107 × 10²⁴ He atoms

Explanation:

To find the number of atoms given the number moles we use the formula

<h3>N = n × L</h3>

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

We have

N = 3.5 × 6.02 × 10²³

We have the final answer as

<h3>2.107 × 10²⁴ He atoms</h3>

Hope this helps you

4 0
3 years ago
What is the average isotopic mass of an element that has the following abundances in nature? Isotopic mass: X20 X22 X23 Abundanc
Paladinen [302]

Answer: 20.2

Explanation:

Mass of isotope 1 = 20

% abundance of isotope 1 = 90.5% = \frac{90.5}{100}=0.905

Mass of isotope 2 = 22

% abundance of isotope 2 = 8.0% = \frac{8}{100}=0.08

Mass of isotope 3 = 23

% abundance of isotope 3 = 1.5% = \frac{1.5}{100}=0.015

Formula used for average atomic mass of an element :

\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}\times {{\text { fractional abundance}})

A=\sum[(20\times 0.905+(22\times 0.08)+(23\times 0.015]

A=20.2

Therefore, the average atomic mass of the element is 20.2.

8 0
3 years ago
The number of protons in a neutral atom is balanced by an equal number of
anastassius [24]
There would be an equal amounts of ELECTRONS.

In order for the atom to be neutral it would imply that the number of protons (positive particles) and the number of electrons (negative particles) are equal since the neutrons are without charge.
3 0
3 years ago
A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The
iVinArrow [24]

Answer:

[NH₃]  → 3.24 M  

Explanation:

Our solute: Ammonia

Our solvent: Water

Solution's mass = Mass of solute + Mass of solvent

Solution's mass = 15 g + 250 g = 265g

We use density to determine, the volume.

D = mass /volume → Volume = m / D →  265 g /0.974 g/mL = 272.07 mL.

We convert the mL to L → 272.07 mL . 1L /1000mL = 0.27207 L

To determine molarity we need the moles of solute in 1 L of solution.

Moles of solute are: 15g / 17g/mol = 0.882 moles

[NH₃] = 0.882mol /0.27207 L → 3.24 M  

3 0
3 years ago
The solubility of KCl is 3.7 M at 20 °C. Two beakers each contain 100. mL of saturated KCl solution: 100. mL of 4.0 M HCl is add
JulijaS [17]

Answer:

a)The Ksp was found to be equal to 13.69

Explanation:

Terminology

Qsp of a dissolving ionic solid — is the solubility product of the concentration of ions in solution.

Ksp however, is the solubility product of the concentration of ions in solution at EQUILIBRIUM with the dissolving ionic solid.

Note that if Qsp > Ksp , the solid at a certain temperature, will precipitate and form solid. That means the equilibrium will shift to the left in order to attain or reach equilibrium (Ksp).

Step-by-step solution:

To solve this: 

#./ Substitute the molar solubility of KCl as given into the ion-product equation to find the Ksp of KCl.

#./ Find the total concentration of ionic chloride in each beaker after the addition of HCl. We pay attention to the amount moles present at the beginning and the moles added.

#./ Find the Qsp value to to know if Ksp is exceeded. If Qsp < Ksp, nothing will precipitate.

a) The equation of solubility equilibrium for KCL is thus;

KCL_(s) ---> K+(aq) + Cl- (aq)

The solubility of KCl given is 3.7 M.

Ksp= [K+][Cl-] = (3.7)(3.7) =13.69

The Ksp was found to be equal to 14.

In pure water KCl

Ksp =13.69 KCl =[K+][Cl-]

Let x= molar solubility [K+],/[Cl-] :. × , x

Ksp =13.69 = [K+][Cl-] = (x)(x) = x²

x= √ 13.69 = 3.7 M moles of KCl requires to make 100mL saturated solutio

37M moles/L

The Ksp was found to be equal to 14.

4.0 M HCl = KCl =[K+][Cl-]

Let y= molar solubility :. y, y+4

Ksp =13.69= [K+][Cl-] = (y)(y*+4)

* - rule of thumb

Ksp =13.69= [K+][Cl-] = (y)(y*+4)= y(4)

13.69=4y:. y= 3.42 moles/100mL

y= 34.2moles/L

8 M HCl = KCl =[K+][Cl-]

Let b= molar solubility :. B, b+8

Ksp =13.69= [K+][Cl-] = (b)(b*+8)

* - rule of thumb

Ksp =13.69= [K+][Cl-] = (b)(b*+8)= b(8)

13.69=8b:. b= 1.71 moles/100mL

17.1 moles/L

Therefore in a solution with a common ion, the solubility of the compound reduces dramatically.

8 0
3 years ago
Read 2 more answers
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