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valentinak56 [21]
3 years ago
13

how does the energy required to sublime a substance compare to the energy required to melt the substance

Chemistry
1 answer:
Darya [45]3 years ago
3 0
The energy required to sublime (solid to gas) a substance at 1 ATM pressure is greater than the energy required to melt (solid to liquid) a substance. When you compare the energies in varying pressures, however, this trend is not always the case. 

<span>any 'general phase diagram', you can see that under the triple point, when all phases are in equilibrium, have solid and gas meeting under a certain pressure. In a vacuum, it would require less energy to sublime than to melt.</span>
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1. A sample of oxygen is collected over water at 22 ° C and 762 torr. What is the partial pressure of the dry oxygen? The vapor
Rom4ik [11]

Answer: The partial pressure of the dry oxygen is 742 torr

Explanation:

Dalton's Law of Partial Pressure states that the total pressure exerted by a mixture of gases is the sum of partial pressure of each individual gas present. Thus P(total)=P_1+P_2 .........

Given; Total pressure = 762 torr

partial pressure of water = 19.8 torr

partial pressure of dry oxygen = ? torr

Total pressure  = partial pressure of water + partial pressure of dry oxygen

762 torr = 19.8 torr = partial pressure of dry oxygen

partial pressure of dry oxygen = 742 torr

The partial pressure of the dry oxygen is 742 torr

8 0
3 years ago
8. As the temperature of a mixture increases, one part of the mixture may 2 points
disa [49]

Answer:

It's false

Explanation:

Mixtures are always combinations of the same compounds that are at different states.

8 0
2 years ago
If a sample of CO gas at 1.977 atm has a volume of 517.4 mL and the pressure is changed to
Mekhanik [1.2K]

Answer:

The answer to your question is V2 = 333.9 ml

Explanation:

Data

Pressure 1 = P1 = 1.977 atm

Volume 1 = V1 = 517.4 ml

Pressure 2 = P2 = 3.063 atm

Volume 2 = V2 = ?

Process

To solve this problem use Boyle's law

              P1V1 = P2V2

-Solve for V2

              V2 = P1V1/P2

-Substitution

              V2 = (1.977 x 517.4) / 3.063

-Simplification

              V2 = 1022.9 / 3.063

-Result

              V2 = 333.9 ml

3 0
3 years ago
How much heat is required to raise the temperature of 10.35g of CCl4 from 32.1°c to 56.4°c
Travka [436]
We are going to use this formula:

Q = M*C*ΔT

when Q is the heat required 

M is the mass of CCl4 = 10.35 g

C is the specific heat capacity of CCl4 = 0.874J/g.c

and ΔT the change in temperature = 56.4 - 32.1 °C =24.3 °C

∴ Q = 10.35g * 0.874 * 24.3 °C

       = 219.8 J
4 0
3 years ago
Which chemical equation is balanced
Norma-Jean [14]

Explanation:

right answer is A

2K + H20 → K20 + H2

5 0
2 years ago
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