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-Dominant- [34]
2 years ago
14

If the specific heat of water is 4. 18 j/g∙°c, how much heat is required to increase the temperature of 1. 20 kg of water from 2

3. 00 °c to 39. 00 °c?
Chemistry
1 answer:
Mkey [24]2 years ago
8 0

The heat required to increase the temperature of 1.20 g of water is  80,256 k/j

<h3>What is specific heat?</h3>

The amount of energy needed to raise the temperature of one gram of a substance by one degree Celsius.

4. 18 J heat is required to change the temperature of 1.20 kg of water from 23. 00 °c to 39. 00 °c.

The heat required to raise temperature is the product of mass, specific heat and temperature change

1,200 × 4.18 × (39 − 23) = 80,256

Thus, the heat required to increase the temperature of 1.20 g of water is  80,256 k/j

Learn more about specific heat

brainly.com/question/11297584

#SPJ4

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borishaifa [10]

1.51 x 10²⁵atoms

Explanation:

Given parameters:

Mass of Na = 578g

Unknown:

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Solution:

 To find the number of atoms, we must first find the number of moles the given mass contains.

  Number of moles  = \frac{mass}{molar mass}

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 Number of moles =  \frac{578}{23} =  25.13moles

   1 mole of a substance = 6.02 x 10²³atoms

    25.13 mole of Na = 25.13 x  6.02 x 10²³atoms

 This gives  1.51 x 10²⁵atoms of Na

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