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Arturiano [62]
3 years ago
9

2.40 kJ of heat is added to a slug of platinum and a separate 2.40 kJ of heat is added to a slug of zinc. The heat capacity of t

he platinum slug is 209J/°C while the heat capacity of the zinc slug is 575 J/°C. ​​​​​​​If the slugs are each originally at 25.00°C, what is the final temperature of each slug?

Chemistry
1 answer:
leonid [27]3 years ago
3 0

Final temperature of platinum :-   36.5°C

Final temperature of Zinc :-  29.17°C


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Electron configuration of Mo
makkiz [27]

Answer:The computer writes electron configurations in the form, for Co for example, [Ar]3d(7)4s(2), which we would write [Ar]3d74s2

NOTE: Write electron configurations as they appear in the periodic table in the front of you text put 4f before 5d

Explanation:

3 0
3 years ago
How much energy is required to convert 15.0 g of ice at −106 °C to water vapor at 125 °C? Specific heats are 2.09 J/g K for both
myrzilka [38]

Answer:

49.3 kJ of energy is required

Explanation:

An exercise of calorimetry at its best

First of all, convert the ice to water before melting.

Q = ice mass . C . ΔT

Q = 15 g . 2.09 J/g°C (0° - (-106°C)

15 g . 2.09 J/g°C . 106°C = 3323.1 J

Now we have to melt the ice, to change its state

Q = mass . latent heat of fusion

Q = 15 g . 0.335 kJ/g = 5.025 kJ .1000 = 5025 J

After that, we have liquid water at 0° and the ice has melted completely. We have to release energy to make a temperature change, to 100° (vaporization)

Q = 15g . 4.18 J/g°C (100°C - 0°C)

Q = 6270 J

Water has been vaporizated so we have to calculate, the state change.

Q = mass . latent heat of vap

Q = 15 g. 2.260 kJ/g

Q = 33.9 kJ (.1000) = 33900 J

Finally we have to increase temperature from 100°C to 125°C

Q = 15 g . 2.09 J/g°C . (125°C - 100°C)

Q = 783.75 J

To know how much energy is required to conver 15 g of ice, to water vapor at 125°C, just sum all the heat released.

3323.1 J + 5025 J + 6270 J + 33900 J + 783.75 J = 49301.85 joules.

Notice I have to convert kJ to J in two calcules to make the sum.

49301.85 joules / 1000 = 49.3 kJ

4 0
3 years ago
3. Skunks run about 10 miles per hour and won't try to outrun a predator. Instead, they
Andrej [43]

Answer:

heelpindgbsjdjfjfhjf d drrr¾rereerrrr. freee points

4 0
2 years ago
How much energy is required to heat a frozen can of juice (360 grams- mostly water) from 0 degrees Celsius ( the temperature of
Usimov [2.4K]

Answer:

1,100,160J or 262.94 kcal

Explanation:

The juice is frozen at 0 degrees Celsius and I assume that it will become gas at 100 degrees Celsius. So we change the form of the water from solid to liquid, then to gas. That means we have to find out how much heat needed to change water form too, not only the heat needed to increase its temperature.

The latent heat of water is 4.2J/g °C while the heat of fusion is 334 J/g and the heat of vaporization is 2260 J/g. The energy needed will be:

360g * 4.2J/g °C * (110-0°C ) + 360g * 334 J/g + 360g * 2260 /g = 1,100,160J or 262.94 kcal.

8 0
3 years ago
What is the molar mass of an element?
Vesnalui [34]

The answer is: the mass of 6.02 x 1023 representative particles of the element.

The base SI unit for molar mass is kg/mol, but chemist more use g/mol (gram per mole).

For example, molar mas of ammonia is 17.031 g/mol.

M(NH₃) = Ar(N) + 3 · Ar(H) · g/mol.

M(NH₃) = 14.007 + 3 · 1.008 · g/mol.

M(NH₃) = 17.031 g/mol.

The molar mass (M) is the mass of a given substance (in this example ammonia) divided by the amount of substance.


8 0
3 years ago
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