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3 years ago

How are isotopes defined?

Chemistry

2 answers:

Setler79 [48]3 years ago

5 0

Answer: it forms of the same element that differ in the number of neutrons in each atom.

or letter c. if on edg

thank me later XD

Alla [95]3 years ago

3 0

Isotopes are atoms with the same number of protons and electrons but different number of neutrons.

Extra for better understanding:
Thus, the relative atomic mass (Ar) differs amongst the isotope. For example, Chlorine have 2 main isotopes with Ar of 35 and 37. The chemical property of the isotopes is the same but the physical property such as boiling point may change.

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Please write down the definitions of elements, compounds, mixtures, homogenous mixtures, and heterogenous mixtures.

MA_775_DIABLO [31]

A homogeneous mixture is a mixture in which the composition is uniform throughout the mixture.

A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture.

3 0

3 years ago

Read 2 more answers

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.184 s^-1 ? Suppose a vessel contai

meriva

Answer:

0.57 M

Explanation:

rate = change in concentration /time

Initial concentration of Cl2O5 = 1.16 M

Let the concentration of Cl2O5 after 5.70 seconds be y

rate = (1.16 - y)/5.7

The reaction follows a first order

Therefore, rate = ky = 0.184y

0.184y = (1.16 - y)/5.7

0.184y × 5.7 = 1.16 - y

1.0488y + y = 1.16

2.0488y = 1.16

y = 1.16/2.0488 = 0.57 M

Concentration of Cl2O5 after 5.70 seconds is 0.57 M

6 0

4 years ago

If the initial volume is 55ml and the final volume after some rocks of sandstone are added is 65ml what is the volume of the chi

AfilCa [17]

Answer:

Volume = 10ml

Density = 1/5 g/ml or 0.20g/ml

Explanation:

The rocks are 10ml since the initial volume went up by 10.

Since density = mass/volume, you divide 2 by 10.

D = 2/10

D = 1/5 g/ml or 0.20g/ml

(Unit is g/ml aka grams/millileter)

7 0

3 years ago

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation:

rusak2 [61]

Answer:

60.42% is the percent yield of the reaction.

Explanation:

Moles of methane gas at 734 Torr and a temperature of 25 °C.

Volume of methane gas = V = 26.0 L

Pressure of the methane gas = P = 734 Torr = 0.9542 atm

Temperature of the methane gas = T = 25 °C = 298.15 K

Moles of methane gas = n

$PV=nRT$

$n=\frac{PV}{RT}=\frac{0.9542 atm\times 26.0L}{0.0821 atm L/mol K\times 298.15 K}=1.0135 mol$

Moles of water vapors at 700 Torr and a temperature of 125 °C.

Volume of water vapor = V' = 23.0 L

Pressure of water vapor = P' = 700 Torr = 0.9100 atm

Temperature of water vapor = T' = 125 °C = 398.15 K

Moles of water vapor gas = n'

$P'V'=n'RT'$

$n'=\frac{PV}{RT}=\frac{0.9100 atm\times 23.0L}{0.0821 atm L/mol K\times 398.15 K}=0.6402 mol$

$CH_4(g)+H_2O(g)\rightarrow CO(g)+3H_2(g)$

According to reaction , 1 mol of methane reacts with 1 mol of water vapor. As we can see that moles of water vapors are in lessor amount which means it is a limiting reagent and formation of hydrogen gas will depend upon moles of water vapors.

According to reaction 1 mol of water vapor gives 3 moles of hydrogen gas.

Then 0.6402 moles of water vapor will give:

$\frac{3}{1}\times 0.6402 mol=1.9208 mol$ of hydrogen gas