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trapecia [35]
2 years ago
7

Which of the following is not a use of radioactive isotopes?

Chemistry
2 answers:
ANEK [815]2 years ago
8 0

Answer:

i belive the answer you are looking for is A.. hope this helps!

Explanation:

im not really 100% certain of this answer due to the fact i am a little rusty.

madreJ [45]2 years ago
5 0
Its A ‏ Believe me I got it on the test
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The strongest light left over from the big bang is called background radiation and was given off as which type of wave?
Sonja [21]
It would be Microwaves. The cosmic microwave background (CMB, CMBR), in Big Bang cosmology, is electromagnetic radiation as a remnant from an early stage of the universe, also known as "relic radiation".
8 0
3 years ago
How many moles are in 23.8 g of sulfur dioxide
Yuki888 [10]

Answer:

0.371

Explanation:

number of moles = mass / Ar

= 23.8g / 32.1 + (16.0 × 2)

= 0.37129485179 = 0.371 (3 s.f).

hope it helps :)

4 0
2 years ago
Give the volume indicated. Be sure to include all significant figures.<br> 9.2<br> 9.16<br> 9.26
Gemiola [76]

Answer:

The volume indicated would be closest to 9.16

3 0
3 years ago
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If a reaction mixture contains only n 2o and no2 at partial pressures of 1.0 atm each the reaction will be spontaneous until som
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4 0
3 years ago
A container of N2O3(g) has a pressure of 0.265 atm. When the absolute temperature of the N2O3(g) is tripled, the gas completely
Rzqust [24]

Answer:

1.59 atm

Explanation:

The reaction is:

N_{2}O_{3}(g) - - -> NO_{2}(g)+NO(g)

The dalton's law tell us that the total pressure of a mixture of gases is the sum of the partial pressure of every gas.

So after the reaction the total pressure is:

P_{total}=P_{NO_{2}}+P_{NO}

we don't include N_{2}O_{3} because it decomposed completely.

Assuming  ideal gases

PV=nRT

P= pressure, V= volume of the container, n= mol of gas, R=constant of gases and T=temperature.

so moles of N_{2}O_{3} is:

n_{N_{2}O_{3}}=\frac{P_{1}V}{RT_{1}}

from the  reaction stoichiometry (1:1) we have that after the reaction the number of moles of each product is the same number of moles of N_{2}O_{3}.

n_{NO_{2}}=\frac{P_{1}V}{RT_{1}}

n_{NO}=\frac{P_{1}V}{RT_{1}}

The partial pressure of each gas is:

P_{NO_{2}}=\frac{n_{NO_{2}*R*T_{2}}}{V}

P_{NO}=\frac{n_{NO}*R*T_{2}}{V}

so total pressure is:

P_{total}=(n_{NO_{2}}+n_{NO})*\frac{R*T_{2}}{V}

replacing the moles we get:

P_{total}=(2*\frac{P_{1}V}{RT_{1}})*\frac{R*T_{2}}{V}

We know that T2=3*T1

replacing this value in the equation we get:

P_{total}=2*\frac{P_{1}V}{RT_{1}}*\frac{R*3T_{1}}{V}

P_{total}=6*P_{1} = 6*0.265 atm = 1.59 atm

5 0
3 years ago
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