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3 years ago

Give evidence to support or dispute: “In nature, the chance of finding one isotope of an element is the same for all elements.”

Chemistry

1 answer:

alekssr [168]3 years ago

5 0

Answer:

False, isotopes have different occurrence percentages, so the changes are different.

Explanation:

Hello,

In this case, since it is false that the isotopes of all the elements can be found with the same chance (occurrence) we can consider the following facts:

1. Carbon atom has two major occurring isotopes: C-12 (98.93%) and C-13 (1.07%).

2. Bromine atom has two major occurring isotopes: Br-79 (50.69%) and Br-81 (49.31%).

3. Calcium has four major occurring isotopes: Ca-40 (96.941%), Ca-42 (0.647%), Ca-43 (0.135%) and Ca-44 (2.086%).

Which show us that the chances of finding any isotope differ among elements.

Regards.

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What is the mass of 3.01x1023 atoms of iron(atomic mass of fe=56)

nlexa [21]

Answer:

N = n× l

N = number of entities

n= moles

l = Avogadro's constant = 6.023 × 10^23

3.01 × 10^ 23 = n * 6.023 × 10^23

n = 3.01 × 10^23/6.023 × 10^23

n= 0.5moles

Molar mass = mass/ number of moles

Molar mass = 56

mass = 56 × 0.5

= 28g

Hope this helps.

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4 years ago

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A mixture of N2, O2, and Ar has mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pr

s344n2d4d5 [400]

Answer:

Partial pressure of nitrogen gas is 0.98 bar.

Explanation:

According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gases.

$P=p_{N_2}+p_{O_2}+p_{Ar}$

$p_{N_2}=P\times \chi_{N_2}$

$p_{O_2}=P\times \chi_{O_2}$

$p_{Ar}=P\times \chi_{Ar}$

where,

$P$ = total pressure = 3.9 bar

$p_{N_2}$ = partial pressure of nitrogen gas

$p_{O_2}$ = partial pressure of oxygen gas

$p_{Ar}$ = partial pressure of argon gases

$\chi_{N_2}$ = Mole fraction of nitrogen gas = 0.25

$\chi_{O_2}$ = Mole fraction of oxygen gas = 0.65

$\chi_{Ar}$ = Mole fraction of argon gases = 0.10

Partial pressure of nitrogen gas :

$p_{N_2}=P\times \chi_{N_2}=3.9 bar\times 0.25 =0.98 bar$

Partial pressure of oxygen gas :

$p_{N_2}=P\times \chi_{O_2}=3.9 bar\times 0.65=2.54 bar$

Partial pressure of argon gas :

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4 years ago

What is S for the reaction N2(g) +O2(g) 2NO? Use G = 173.3 kJ at 303.0 K and H = 180.7 kJ. Use G = H – TS.

Rashid [163]

Given information :

G = 173.3 KJ

H = 180.7 KJ

T = 303.0 K

S = unknown (?)

By using the given formula : G = H - TS , we can calculate the value of 'S'

On rearranging the formula we get : S = $\frac{H-G}{T}$

Plug in the value of G , H and T in the above formula :

S = $\frac{(180.7 KJ - 173.3KJ)}{303.0K}$

S = 0.02442 $\frac{KJ}{K}$

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