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Svetradugi [14.3K]
3 years ago
14

The barium isotope 133ba has a half-life of 10.5 years. a sample begins with 1.1×1010 133ba atoms. how many are left after (a) 5

years, (b) 30 years, and (c) 190 years?
Chemistry
2 answers:
enot [183]3 years ago
7 0

Answer: Atoms of _{56}^{133}\textrm{Ba} left in

a) N=78.608\times 10^8atoms

b) N=14.650\times 10^8atoms

c) N=31.35\times 10^3atoms

Explanation: The given reaction is a type of radioactive decay and all the radioactive decay follows first order reactions. Hence, to calculate the rate constant, we use the formula:

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

t_{1/2}=10.5years

k=\frac{0.693}{10.3years}\\k=0.0672years^{-1}

To calculate how much amount of sample is left, we use the rate law expression for first order kinetics, which is:

N=N_oe^{-kt}    ....(1)

where,

k = rate constant  = 0.0672years^{-1}

t = time taken for decay process

N_o = initial amount of the reactant  = 1.1\times 10^{10}g

N = amount left after decay process

  • For a)

t = 5 years

Putting values in equation 1, we get:

N=(1.1\times 10^{10})\times e^{(-0.0672years^{-1}\times 5years)}\\N=78.608\times 10^8atoms

  • For b)

t = 30 years

Putting values in equation 1, we get:

N=(1.1\times 10^{10})\times e^{(-0.0672years^{-1}\times 30years)}\\N=14.650\times 10^8atoms

  • For c)

t = 190 years

Putting values in equation 1, we get:

N=(1.1\times 10^{10})\times e^{(-0.0672years^{-1}\times 190years)}\\N=31.35\times 10^3atoms

Sladkaya [172]3 years ago
4 0
<span>a) 7.9x10^9 b) 1.5x10^9 c) 3.9x10^4 To determine what percentage of an isotope remains after a given length of time, you can use the formula p = 2^(-x) where p = percentage remaining x = number of half lives expired. The number of half lives expired is simply x = t/h where x = number of half lives expired t = time spent h = length of half life. So the overall formula becomes p = 2^(-t/h) And since we're starting with 1.1x10^10 atoms, we can simply multiply that by the percentage. So, the answers rounding to 2 significant figures are: a) 1.1x10^10 * 2^(-5/10.5) = 1.1x10^10 * 0.718873349 = 7.9x10^9 b) 1.1x10^10 * 2^(-30/10.5) = 1.1x10^10 * 0.138011189 = 1.5x10^9 c) 1.1x10^10 * 2^(-190/10.5) = 1.1x10^10 * 3.57101x10^-6 = 3.9x10^4</span>
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Answer: The given statement is true.

Explanation:

According to the Dalton's law, total pressure of a mixture of gases that do not react with each other is equal to the partial pressure exerted by each gas.

The relationship is as follows.

          p_{total} = \sum_{i=1}^{n} p_{i}

or,        p_{total} = p_{1} + p_{2} + p_{3} + p_{4} + ......... + p_{n}

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Also, relation between partial pressure and mole fraction is as follows.

                 p_{i} = p_{total} \times x_{i}

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Question List (4 items) (Drag and drop into the appropriate area) Find the volume of HCl that will neutralize the base. Find the
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The question is incomplete, the complete question is:

The solubility of slaked lime, Ca(OH)_2, in water is 0.185 g/100 ml. You will need to calculate the volume of 2.50\times 10^{-3}M HCl needed to neutralize 14.5 mL of a saturated

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<u>Explanation:</u>

Given values:

Solubility of Ca(OH)_2 = 0.185 g/100 mL

Volume of Ca(OH)_2 = 14.5 mL

Using unitary method:

In 100 mL, the mass of Ca(OH)_2 present is 0.185 g

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The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

Given mass of Ca(OH)_2 = 0.0268 g

Molar mass of Ca(OH)_2 = 74 g/mol

Plugging values in equation 1:

\text{Moles of }Ca(OH)_2=\frac{0.0268g}{74g/mol}=0.000362 mol

Moles of OH^- present = (2\times 0.000362)=0.000724mol

The chemical equation for the neutralization of calcium hydroxide and HCl follows:

Ca(OH)_2+2HCl\rightarrow CaCl_2+2H_2O

By the stoichiometry of the reaction:

Moles of OH^- = Moles of H^+ = 0.000724 mol

The formula used to calculate molarity:

\text{Molarity of solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (mL)}} .....(2)

Moles of HCl = 0.000724 mol

Molarity of HCl = 2.50\times 10^{-3}

Putting values in equation 2, we get:

2.50\times 10^{-3}mol=\frac{0.000724\times 1000}{\text{Volume of solution}}\\\\\text{Volume of solution}=\frac{0.000725\times 1000}{2.50\times 10^{-3}}=290mL

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Answer:

The correct answer is D

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<u></u>

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This is calculated by using :

Molecular weight = number of atom x atomic mass of the atom

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