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2 years ago

15

The isotope 226Ra has a half-life for radioactive decay of 1600 Y. How long will it take the amount of 226 Ra in a sample of 226

RaCl2 to decrease by 25%

1 answer:

Nostrana [21]2 years ago

8 0

The correct answer is 226Ra is half and long as radioactive decay

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A compound colors flames violet what could it contain

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<span>Caesium is a possibility; the flame test for caesium is said to beblue-violet, though I've never actually seen it so I'm not sure howblue or how.</span>

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3 years ago

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3 years ago

How is the Law of Conservation of Mass, Matter, Phases of Matter, and Physical/Chemical Changes similar/connected to one another

kogti [31]

Answer:

Solids, liquids, and gases are made of tiny particles called atoms and molecules. In a solid, the particles are very attracted to each other. They are close together and vibrate in position but don't move past one another. In a liquid, the particles are attracted to each other but not as much as they are in a solid.

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3 years ago

Convert 7.2 × 10^23 molecules of CO2 to moles (round to the nearest tenth). <br>Unit?

Svetach [21]

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x ___________________

6.02* 10^23 molecules CO2

=1.196

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3 years ago

The mass percent of Cl⁻ in a seawater sample is determined by titrating 25.00 mL of seawater with AgNO₃ solution, causing a prec

Serga [27]

Answer:

2.5 %

Explanation:

Considering:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

Or,

$Moles =Molarity \times {Volume\ of\ the\ solution}$

Given :

For $AgNO_3$ :

Molarity = 0.2850 M

Volume = 63.30 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 63.30 × 10⁻³ L

Thus, moles of $AgNO_3$ :

$Moles=0.2850 \times {63.30\times 10^{-3}}\ moles$

Moles of $AgNO_3$ = 0.0180405 moles

Moles of $AgNO_3$ = Moles of $Cl^-$

Thus, Moles of $Cl^-$ = 0.0180405 moles

Molar mass of $Cl^-$ = 35.453 g/mol

Mass = Moles * Molar mass = 0.0180405 moles * 35.453 g/mol = 0.6396 g

Volume of sea water = 25.00 mL

Density = 1.024 g/mL

Density = Mass / Volume

Mass = Density * Volume = 1.024 g/mL * 25.00 mL = 25.6 g

$Mass\ \%=\frac{Mass_{Chloride ion}}{Total\ mass}\times 100$

$Mass\ \%=\frac{0.6396}{25.6}\times 100$

<u>Mass percent of Cl⁻ = 2.5 %</u>

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3 years ago