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mario62 [17]
3 years ago
11

Calculate the energy needed to raise the temperature of 165.0 g of water from 10.0°C to 40.0°C. The specific heat capacity for w

ater is 4.2J/g °C.
Chemistry
1 answer:
mr Goodwill [35]3 years ago
7 0

Answer:

20790 J

Explanation:

From the question given above, the following data were obtained:

Mass (M) = 165 g.

Initial temperature (T1) 10 °C.

Final temperature (T2) = 40 °C.

Specific heat capacity (C) = 4.2 J/g °C.

Heat (Q) required =?

Next, we shall determine the change in temperature of water. This can be obtained as illustrated below:

Initial temperature (T1) 10 °C.

Final temperature (T2) = 40 °C.

Change in temperature (ΔT) =?

ΔT = T2 – T1

ΔT = 40 – 10

ΔT = 30 °C

Finally, we shall determine the heat energy required to raise the temperature of the water as follow:

Mass (M) = 165 g.

Specific heat capacity (C) = 4.2 J/g °C.

Change in temperature (ΔT) = 30 °C

Heat (Q) required =?

Q = MCΔT

Q = 165 × 4.2 × 30

Q = 20790 J

Thus, the heat energy required to raise the temperature of the water is 20790 J

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Explanation:

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if only 0.264 g of ca(oh)2 dissolves in enough water to give 0.178 l of aqueous solution at a given temperature, what is the ksp
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The ksp value for calcium hydroxide at this temperature is 5.20 × 10⁻⁶.

<h3>What is ksp?</h3>

Ksp is an equilibrium constant of a solid substance dissolved in a liquid solution.

Given that, the volume of water is 0.178 l, 0.264 g of Ca(OH)² dissolves in enough water

The solution equilibrium is

Ca(OH)² = Ca + 2OH

The molar solubility is

0.186 / 74.00  / 0.230 = 0.0109 M

The ksp value will be

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Putting the values in the formula

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To learn more about ksp value, refer to the link:

brainly.com/question/27132799

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Let’s say that the initial concentration of SrSo4 was 1. ( or we have 1 mole of this reagent).

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