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Murljashka [212]
3 years ago
13

A sample contains 25% parent isotope and 75% daughter isotopes. If the half-life of the parent isotope is 72 years, how old is t

he sample?
Chemistry
2 answers:
Mrrafil [7]3 years ago
7 0

Answer: The sample is 144 years old.

Explanation: This is a type of radioactive decay and all radioactive decays follow first order kinetics.

We are given half life which is 72 years.  

To calculate the rate constant, we use the formula:

k=\frac{0.693}{t_{1/2}}

k=\frac{0.693}{72years}

k=0.0096years^{-1}

Also 25 % of parent isotope is left, that means 75 % has been decomposed

Expression for rate law for first order kinetics is given by:

k=\frac{2.303}{t}\log\frac{a}{a-x}

where,

k = rate constant

t = time taken for decay process

a = initial amount of the reactant  = parent isotope= 100

a - x = amount left after decay process  = 25

Putting values in above equation, we get:

0.0096years^{-1}=\frac{2.303}{t}\log\frac{100}{25g}

t=144years

alisha [4.7K]3 years ago
5 0

The radioactive decay obeys first order kinetics

the rate law expression for radioactive decay is

ln\frac{[A_{0}]}{[A_{t}]}=kt

Where

A0 = initial concentration

At = concentration after time "t"

t = time

k = rate constant

For first order reaction the relation between rate constant and half life is:

k=\frac{0.693}{t_{\frac{1}{2} } }

Let us calculate k

k = 0.693 / 72 = 0.009625 years⁻¹

Given

At = 0.25 A0

ln(\frac{A0}{0.25A0})=0.009625  X time

time = 144 years

So after 144 years the sample contains 25% parent isotope and 75% daughter isotopes**

Simply two half lives

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A sample of the mineral hematite Iron (III) oxide has a mass of 12.4g. How many moles of the mineral are present?
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Thus problem is providing us with the mass of iron (III) oxide as 12.4 g so the moles are required and found to be 0.0776 mol after the calculations:

<h3>Mole-mass relationships:</h3>

In chemistry, we use mole-mass relationships in order to calculate grams from moles and vice versa. In this case, since we are given the mass of iron (III) oxide as 12.4 g one can calculate the moles by firstly quantifying its molar mass:

Fe_2O_3\rightarrow 2*55.85 g/mol+3*16.00 g/mol=159.7g/mol

Then, we prepare a conversion factor in order to cancel out the grams and thus, get moles:

12.4gFe_2O_3*\frac{1molFe_2O_3}{159.7gFe_2O_3} \\\\=0.0776molFe_2O_3

Learn more about mole-mass relationships: brainly.com/question/18311376

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Which components of a galaxy move in circular patterns or revolve around a star?
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Dalton hypothesized that atoms are indivisible and that all atoms of an element are identical. It is now known that _____.
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Dalton hypothesized that atoms are indivisible and that all atoms of an element are identical. It is now known that <span>atoms are divisible. The answer is letter C</span>
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What mass of carbon dioxide is formed when 1.75 mol of ethane burns completely in oxygen?
dybincka [34]

Answer:

There is a mass of 154 Grams of Carbon Dioxide.

Explanation:

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This means we have 1.05 X 10^24 total particles of Ethane.

Each ethane particle contains 2 carbon atoms.

If every particle of ethane is burned, we will end up with 2.10 x 10^24 molecules of Carbon Dioxide (Particles of Methane x 2, since each Methane particle contains 2 carbon atoms)

Carbon Dioxide has a molar mass of 44.01 g/mol

So if we take our amount of Carbon Dioxide molecules and divide it by 1 mole, ((2.10 x 10^24)/(6.02 x 10^23) = 3.49) we find that we have 3.49 moles of Carbon Dioxide.

Now all we need to do is multiply our moles of carbon dioxide(3.49) by it's molar mass(44.01) while accounting for significant digits.

What you should end up with is 154 Grams of Carbon Dioxide.

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3 0
3 years ago
If 4.50 l of water vapor at 50.2 °c and 0.121 atm reacts with excess iron, how many grams of iron(iii) oxide will be produced?
Flura [38]
When the balanced equation for this reaction is:
2Fe + 3H2O → Fe2O3  +  3H2

and according to the vapour pressure formula:
PV= nRT
when we have P is the vapor pressure of H2O= 0.121 atm
and V is the volume of H2O = 4.5 L
and T in Kelvin = 52.5 +273 = 325.5 K
R= 0.08205 atm-L/g mol-K
So we can get n H2O
So, by substitution:
n H2O = PV/RT
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we can get the Mass of Fe2O3 from this formula:
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∴ 1.084 gm of Fe2O3 will produced
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4 years ago
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