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77julia77 [94]
2 years ago
12

Which statement defines specific heat capacity for given sample?

Chemistry
2 answers:
ludmilkaskok [199]2 years ago
7 0

Answer:

D. the quantity of heat that is required to raise 1 g of the sample by 1*C (kelvin) at a constant pressure.

Explanation:

took the test

Aleks04 [339]2 years ago
6 0

Answer:

D. the quantity of heat that is required to raise 1 g of the sample by 1*C (kelvin) at a constant pressure.

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Explain how two object create heat went rub quickly
sergiy2304 [10]

Answer:

friction

Explanation:

the resistance that one surface or object encounters when moving over another.

4 0
2 years ago
Why is the composition of the vapor different from the composition of the solution?
BaLLatris [955]
If there is solution with nonvolatile solute (<span>substance that does not readily </span>evaporate<span> into a </span>gas) <span>only the pure vapor of the solvent is present above the solution and solute stays in solution and do not enters vapor above solution. This is because nonvolatile solute has slow rate of evaporation and low vapore pressure.
If solution has two volatile components, composition of the vapor depends on vapor pressures of the components according </span><span>Raoult's Law.</span>
8 0
3 years ago
Hợp chất nào có khả năng là hợp chất ion cao nhất ?<br>A Al2O3<br>B ScCl3<br>C NO2<br>D CCl4
Rzqust [24]

Answer:

B

Explanation:

hợp chất nào có khả năng là hợp chất ion cao nhất ?

A Al2O3?

B

7 0
3 years ago
What happens to the balloons volume as it rises into the atmosphere
ra1l [238]

Answer:

As balloons rise, air pressure around them diminishes. When the ballon is made of elastic material, it expands because of the excess pressure inside. Its volume increases and its internal pressure decreases

Explanation:

8 0
3 years ago
What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
Mariulka [41]

Hey There!

Moles of solution = 7.0 moles

Volume in liters:

569 mL / 1000 => 0.569 L

Therefore:

M = n / V

M = 7.0 / 0.569

= 12.30 M

Hope that  helps!

5 0
3 years ago
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