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leonid [27]
2 years ago
7

What is the half-life of a radioisotope if 25.0 grams of an original 200.-gram sample of the isotope remains unchanged after 11.

46 days?
(1) 2.87 d (3) 11.46 d
(2) 3.82 d (4) 34.38 d
Chemistry
2 answers:
erastova [34]2 years ago
7 0
1. 200/2=100. 100/2=50. 50/2=25. So that's 3 to get to 25. 

2. 11.46/3=3.82

The answer is (2).
andreev551 [17]2 years ago
4 0

Answer : The correct option is, (2) 3.82 d

Solution : Given,

As we know that the radioactive decays follow first order kinetics.

So, the 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  = 11.46 days

a = initial amount of the reactant  = 200 g

a - x = amount left after decay process  = 25 g

Putting values in above equation, we get the value of rate constant.

k=\frac{2.303}{11.46}\log\frac{200}{25}=0.1814

Now we have to calculate the half life of a radioisotope.

Formula used : t_{1/2}=\frac{0.693}{k}

Putting value of 'k' in this formula, we get the half life.

t_{1/2}=\frac{0.693}{0.1814}=3.820

Therefore, the half-life of a radioisotope is, 3.820 d

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Answer:

\large \boxed{109.17 \, ^{\circ}\text{C}}

Explanation:

Data:

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Calculations:

The formula for the boiling point elevation ΔTb is

\Delta T_{b} = iK_{b}b

i is the van’t Hoff factor —  the number of moles of particles you get from 1 mol of solute. For EG, i = 1.

1. Moles of EG

\rm n = 0.50 \times \text{4.70 gal} \times \dfrac{\text{3.785 L}}{\text{1  gal}} \times \dfrac{\text{1000 mL}}{\text{1 L}} \times \dfrac{\text{1.11 g}}{\text{1 mL}} \times \dfrac{\text{1 mol}}{\text{62.07 g}} = \text{159 mol}

2. Kilograms of water

m = 0.50 \times \text{4.70 gal} \times \dfrac{\text{3.785 L}}{\text{1  gal}} \times \dfrac{\text{998 g}}{\text{1 L}} \times \dfrac{\text{1 kg}}{\text{1000 g}} = \text{8.88 kg}

3. Molal concentration of EG

b =  \dfrac{\text{159 mol}}{\text{8.88 kg}} = \text{17.9 mol/kg}

4. Increase in boiling point

\rm \Delta T_{b} = iK_{b}b = 1 \times 0.512 \, \, ^{\circ}\text{C} \cdot kg \cdot mol^{-1} \, \times 17.9 \cdot mol \cdot kg^{-1} = 9.17 \, ^{\circ}\text{C}

5. Boiling point

\rm T_{b} = T_{b}^{\circ} + \Delta T_{b} = 100.00 \, ^{\circ}\text{C} + 9.17 \, ^{\circ}\text{C} = \mathbf{109.17 \, ^{\circ}C}\\\rm \text{The boiling point of the solution is $\large \boxed{\mathbf{109.17 \, ^{\circ}C}}$}

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1. If 22.5 L of nitrogen at 734 mm Hg are compressed to 702 mm Hg at constant
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The answer to your question is   V2 = 23.52 l

Explanation:

Data

Volume 1 = V1 = 22.5 l

Pressure 1 = P1 = 734 mmHg

Volume 2 = V2 = ?

Pressure 2 = 702 mmHg

Process

To solve this problem use Boyle's law.

                      P1V1 = P2V2

-Solve for V2

                          V2 = P1V1 / P2

-Substitution

                          V2 = (734 x 22.5) / 702

-Simplification

                           V2 = 16515 / 702

-Result

                           V2 = 23.52 l

-Conclusion

If we diminish the pressure, the volume will be higher.

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