All categories

3 years ago

What are particles that differ in number between isotopes

Chemistry

1 answer:

balandron [24]3 years ago

7 0

Answer:

Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons and electrons. The difference in the number of neutrons between the various isotopes of an element means that the various isotopes have different masses.

You might be interested in

The ksp of cadmium hydroxide, cd(oh)2, is 7.20 × 10-15. calculate the solubility of this compound in g/l.

olga nikolaevna [1]

When the solubility is the amount of solute that dissolved in a unit volume of the solvent.

and when the balanced reaction equation is:

so, by using the ICE table:

Cd(OH)2(s) ↔ Cd2+ + 2OH-

initial 0 0

change +X +2X

Equ X 2X

so the Ksp expression = [Cd2+] [OH-]^2

and we have Ksp = 7.2 x 10^-15

and when we assume the solubility = X

by substitution:

7.2 x 10^-15 = (X) (2X)^2

7.2 x 10^-15 = X*4X^2

7.2 x 10^-15 = 4X^3

∴X = ∛(7.2x10^-15)/4

= 1.22 x 10^-5 M

∴ the solubility = X = 1.22 x 10^-5 M

6 0

3 years ago

A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 4250 mL of water at 2

Assoli18 [71]

Answer:

The specific heat of copper is 0.385 J/g°C

Explanation:

A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 425 mL of water at 22.55 degrees Celsius. The final temperature of the water was recorded to be 26.15 degrees Celsius. What is the specific heat of the copper?

Step 1: Data given

Mass of copper = 85.2 grams

Temperature of copper = 221.32 °C

Volume of water = 425 mL

Temperature of water = 22.55 °C

Final temperature = 26.15 °C

Specific heat of water = 4.184 J/g°C

Step 2: Calculat the specific heat of copper

Heat lost = heat gained

Q = m*c*ΔT

Qcopper = -Qwater

m(copper)*c(copper)*ΔT(copper) = - m(water) * c(water) * ΔT(water)

⇒ m(copper) = 85.2 grams

⇒ c(copper) = TO BE DETERMINED

⇒ ΔT(copper) = the change in temeprature = T2 -T1 = 26.15 -221.32 = -195.17 °C

⇒ m(water) = The mass of water = 425 mL * 1g/mL = 425 grams

⇒ c(water) = The specific heat of water = 4.184 J/g°C

⇒ ΔT(water) = The change of temperature of water = 26.15 - 22.55 = 3.6

85.2 * c(copper) * (-195.17) = -425 * 4.184 * 3.6

c(copper) = 0.385 J/g°C

The specific heat of copper is 0.385 J/g°C

(Note, The original question says the volume of the water is 4250 mL. IF this is not an error, the specific heat of copper is 3.85 J/g°C (10x higher than the normal value).

8 0

3 years ago

Favorable (Exergonic) chemical reactions:

artcher [175]

Answer:

Usually give off heat energy

Explanation:

Exergonic reactions are the ones which are spontaneous. Spontaneous reactions are indicated by the negative change in the Gibbs free energy. In order to provide characteristics for an exergonic reaction, we need to define the Gibbs free energy in terms of the enthalpy change and the entropy change:

$\Delta G=\Delta H-T\Delta S$

Here:

$\Delta H$ is the enthalpy change;

$\Delta S$ is the entropy change;

$T$ is the absolute temperature.

In order to achieve a negative value in the Gibbs free energy change, we should have:

$\Delta H - T\Delta S$

This is true for all temperatures if:

$\Delta H < 0, \Delta S > 0$

The major term here is the change in enthalpy, notice that we wish the enthalpy change to be negative.

Negative enthalpy change corresponds to an exothermic reaction, the one which releases heat. This means exergonic reactions would usually give off heat.

4 0

3 years ago

using the symbol M for the element, write the chemical formula for the compound that forms when element M reacts with iodine.

Anon25 [30]

Answer : The chemical formula for the compound is, $MI$