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den301095 [7]
3 years ago
10

135 Joules of heat are required to increase the temperature of 10.0 grams of an unknown metal from 25.0∘C to 40.0∘C:

Chemistry
1 answer:
Sever21 [200]3 years ago
8 0

Answer:

270 Joules

Explanation:

The specific heat capacity equation will be used for this question i.e.

Q = m. c. ΔT

Where; Q = Amount of heat

m = mass of substance

C = specific heat capacity of

substance

ΔT = change in temperature

(Final temp - initial temp)

However, for this unknown metal, we need to find the specific heat first by saying; C = Q / mΔT

Q= 135J, C=?, m= 10g, ΔT = (40-25 = 15°C)

C = 135 / 15 × 10

C = 135/150

C = 0.9 J/g°C

If the specific heat capacity of the unknown metal is 0.9 J/g°C, then at a mass of 20.0g, and a ΔT of 15°C, the amount of heat needed is:

Q = m. c. ΔT

Q = 20 × 0.9 × (40-25)

Q = 18 × 15

Q = 270J

270 Joules of heat is needed to increase the temperature of 20g of the metal from 25 - 40°C

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7 0
3 years ago
4. How many moles of KBr are found in 3 Liters of 0.4 M solution?
Allisa [31]

There are 1.2 moles of KBr found in 3 Liters of 0.4 M solution.

<h3>HOW TO CALCULATE NUMBER OF MOLES?</h3>

The number of moles of a substance can be calculated by multiplying the molarity by the volume.

No. of moles = Molarity × volume

According to this question, 3L of a KBr solution are contained in a 0.4M.

no. of moles = 3L × 0.4M = 1.2moles

Therefore, there are 1.2 moles of KBr found in 3 Liters of 0.4 M solution.

Learn more about no. of moles at: brainly.com/question/14919968

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