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Tom [10]
2 years ago
10

Determine the total time that must elapse until only ¼ of an original sample of the radioisotope Rn-222 remains unchanged.

Chemistry
1 answer:
Arte-miy333 [17]2 years ago
5 0

Answer:

7.6 days

Explanation:

Radon is a radioactive element and Radon-222 is it's most stable isotope. The half-life of Radon-222 has been found to be approximately 3.8 days.

Let, the initial amount of the Rn-222 = 1 = A

Final amount = \frac{1}{4} = A'

We will use the following relation for calculating time elapsed in the decay

A' = A(\frac{1}{2} )^\frac{t}{t_1_/_2}  }

Thus,

\frac{1}{4} =1(\frac{1}{2} )^\frac{t}{3.8}

We can write is as,

(\frac{1}{2} )^2=(\frac{1}{2} )^\frac{t}{3.8}

Since the base in both sides are equal, powers can also be equal and thus,

2=\frac{t}{3.8}

So, t = 7.6 days

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Calculate the experimental specific heat capacity of an object of mass 1.32 kg, given that the object releases 1.95 kJ of heat w
andreev551 [17]

Answer:

0.076 J/gºC.

Explanation:

From the question given above, the following data were obtained:

Mass (M) of object = 1.32 kg

Heat (Q) released = –1.95 kJ

Change in temperature (ΔT) = –19.5°C (decrease in temperature)

Specific heat capacity (C) =?

Next, we shall convert 1.32 kg to grams (g). This can be obtained as follow:

1 kg = 1000 g

Therefore,

1.32 kg = 1.32 kg × 1000 g / 1 kg

1.32 kg = 1320 g

Next, we shall convert –1.95 kJ to joule (J). This can be obtained as follow:

1 kJ = 1000 J

Therefore,

–1.95 kJ = –1.95 kJ × 1000 / 1 kJ

–1.95 kJ = –1950 J

Finally, we shall determine the specific heat capacity of the object. This can be obtained as follow:

Mass (M) of object = 1320 g

Heat (Q) released = –1950 J

Change in temperature (ΔT) = –19.5°C (decrease in temperature)

Specific heat capacity (C) =?

Q = MCΔT

–1950 = 1320 × C × –19.5

–1950 = –25740 × C

Divide both side by –25740

C = –1950 / –25740

C = 0.076 J/gºC

Thus, the specific heat capacity of the object is 0.076 J/gºC.

4 0
3 years ago
Non metals are acidic in nature explain with an equation ​
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How many grams of gas must be released from a 32.0 L sample of CO2(g) at STP to reduce the volume to 16.6 L at STP?
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Answer:

30.3 g

Explanation:

At STP, 1 mol of any gas will occupy 22.4 L.

With the information above in mind, we <u>calculate how many moles are there in 32.0 L</u>:

  • 32.0 L ÷ 22.4 L/mol = 1.43 mol

Then we <u>calculate how many moles would there be in 16.6 L</u>:

  • 16.6 L ÷ 22.4 L/mol = 0.741 mol

The <u>difference in moles is</u>:

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Finally we <u>convert 0.689 moles of CO₂ into grams</u>, using its <em>molar mass</em>:

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