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1 month ago

Which list of radioisotopes contains an alpha emitter, a beta emitter, and a positron emitter?

Chemistry

2 answers:

alisha [2.9K]1 month ago

6 0

Answer: The correct option is 3.

Explanation: Radioisotopes that emit alpha-particles are termed alpha-emitters. These isotopes undergo alpha-decay.

Those radioisotopes that emit beta-particles $(_{-1}^0\beta )$ are called beta-emitters. They undergo beta-minus decay, in which a neutron converts to a proton and an electron.

Isotopes that emit positrons $(_{+1}^0\beta )$ are known as positron-emitters, undergoing beta-plus decay where a proton becomes a neutron.

From the options given,

Option 1: All three isotopes undergo beta-minus decay.

Option 2: Cs-137 and Tc-99 undergo beta-minus decay.

Fr-220 undergoes alpha-decay.

Option 3: Kr-85 undergoes beta-minus decay.

$_{36}^{85}\textrm{Kr}\rightarrow _{37}^{85}\textrm{Rb}+_{-1}^0\beta$

Ne-19 undergoes positron decay.

$_{10}^{19}\textrm{Ne}\rightarrow _{9}^{19}\textrm{F}+_{+1}^0\beta$

Rn-222 undergoes alpha decay.

$_{86}^{222}\textrm{Rn}\rightarrow _{84}^{218}\textrm{Po}+_{2}^4\alpha$

Option 4: All three isotopes undergo beta-minus decay processes.

Therefore, the correct choice is 3.

eduard [2.7K]1 month ago

4 0

The correct choice is (3): the list contains β-, β+ and α decay types. For (1) the modes are β-, β- and β-. For (2) they are β-, α and β-. For (4) all three are α decay modes.

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In living organisms, C-14 atoms disintegrate at a rate of 15.3 atoms per minute per gram of carbon. A charcoal sample from an ar

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Answer:

The result is "4,241.17 years"

Explanation:

The disintegration rate for C-14 atoms is indicated in $15.3 \frac{atoms}{min-g}$

The dissolution rate of the sample is given by $9.16 \frac{atoms} {min-gram}$

The C-14 proportion within the sample can be determined as per $= \frac {9.16}{15.3} \\\\ = 0.5987$

With a half-life of 5730 years.

Now, we need to compute the number of half-lives (n) that are applicable:

$(\frac{1}{2})^n= A\\\\A= fraction of C-14, which is remaining \\\\(\frac{1}{2})^n= 0.5987 \\\\ n \log 2 = - \log 0.5987\\\\$

$\therefore \\\\ \Rightarrow n= \frac{0.227}{0.3010} \\\\ = 0.740\\$

Thus, the age of the sample is represented as = $n \times\ half-life$

$= 0.740 \times 5730 \ years \\\\=4241.17 \ years\\\\$

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2 months ago

A girl stands on a bathroom scale. In metric units, the scale indicates that her weight is 42

VMariaS [2998]

Explanation:

The scale under her feet exerts an equal force but opposite in direction.

This principle aligns with Newton's third law of motion, which says that "for every action, there is an equal and opposite reaction."

As the girl’s weight presses down on the scale with a force of 42N, the scale responds with an equal upward force in the opposite direction.

The resulting net force is zero, which explains why her weight does not break the scale.

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2 months ago

A 92.8 gram sample of Ba(OH)2•4H2O (barium hydroxide tetrahydrate) is heated until water is released. How many grams of water we

Alekssandra [3086]

According to the periodic table:
the molar mass of barium is 137.2 grams
the molar mass of oxygen is 16 grams
the molar mass of hydrogen is 1 gram

The molar mass of Ba(OH)2 can be calculated as 137.2 + 2(16) + 2(1) = 171.2 grams.
The molar mass of 4H2O is computed as 4 [2(1) + 16] = 72 grams.

Consequently, the molar mass of Ba(OH)2·4H2O is 171.2 + 72 = 243.2 grams.

Therefore, a sample weighing 243.2 grams of <span>barium hydroxide tetrahydrate includes 72 grams of water, meaning that within 92.8 grams, the mass of water would be:
mass of water in 92.8 grams = (92.8 x 72) / 243.2 = 27.474 grams.

Thus, when heating a 92.8 gram sample of Ba(OH)2·4H2O (barium hydroxide tetrahydrate), 27.474 grams of water will be emitted.</span>

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2 months ago

Excess aqueous copper(II) nitrate reacts with aqueous sodium sulfide to produce aqueous sodium nitrate and copper(II) sulfide as

Tems11 [2777]

The question lacks completeness; the full question is:

Determine the theoretical yield:

When excess aqueous copper(II) nitrate reacts with aqueous sodium sulfide, sodium nitrate and copper(II) sulfide precipitate. For this reaction, 469 grams of copper(II) nitrate was combined with 156 grams of sodium sulfide yielding 272 grams of sodium nitrate.

Answer:

The theoretical yield of sodium nitrate is 340 grams.

Explanation:

$Cu(NO_3)_2(aq)+Na_2S(aq)\rightarrow 2NaNO_3(aq)+CuS(s)$