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ziro4ka [17]
2 years ago
15

The temperature of a 100.0 g sample of water is raised from 30degrees celsius to 100.0 degrees celsius. How much energy is requi

red for the temperature change?
Chemistry
1 answer:
worty [1.4K]2 years ago
6 0

Answer:

29260J

Explanation:

Given parameters:

Mass of water sample  = 100g

Initial temperature = 30°C

Final temperature  = 100°C

Unknown:

Energy required for the temperature change = ?

Solution:

The amount of heat required for this temperature change can be derived from the expression below;

     H  = m c (ΔT)

H is the amount of heat energy

m is the mass

c is the specific heat capacity of water  = 4.18J/g°C

ΔT is the change in temperature

Now insert the parameters and solve;

          H  = 100 x 4.18 x (100 - 30)

          H  = 100 x 4.18 x 70 = 29260J

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<em>When you add just borax, the moles of Na²⁺ are twice the moles of borate²⁻, that means 2borate²⁻=Na⁺ </em><em>(1)</em>

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<em>ksp = [borate²⁻] [Na⁺]²</em>

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The moles of HCl that reacts with B₄O₇²⁻ are:

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As two moles of HCl react with 1 mol of B₄O₇²⁻, the moles of B₄O₇²⁻ are:

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The [borate²⁻] is <em>3,00x10⁻³ mol of B₄O₇²⁻/0,00850L = </em><em>0,353M</em>

And [Na⁺] is <em>6,00x10⁻³ mol of Na⁺ / 0,00850L = </em>0,706M

Replacing in the expression of ksp:

ksp = [0,353] [0,706]²

<em>ksp = 0,176</em>

<em></em>

I hope it helps!

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