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LiRa [457]
3 years ago
11

How much energy (in J) is lost when a sample of iron with a mass of 28.3 g cools from 66.0 degrees celsius to 24.0 degrees celsi

us.
Chemistry
1 answer:
pentagon [3]3 years ago
5 0

Answer:

Q = -535 J.

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the lost energy according to the following and generic heat equation:

Q=mC(T_F-T_i)

Thus, since the specific heat of iron is 0.450 in the SI units, we can plug in the mass and temperatures to obtain:

Q=28.3g*0.450\frac{J}{g\°C} (24.0\°C-66.0\°C)\\\\Q=-535J

Regards

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Answer:

29 mL

Explanation:

<h3>Equation</h3>

The question needs us to find the volume of the liquid. The equation for volume using density and mass is:

Volume = Mass / Density

<h3>Solve</h3>

We can substitute the given values for density and mass into the equation:

V=\frac{25\ g}{0.87\ g/ml}

V\approx29\ mL

<h3>Additional Comments</h3>

The answer we obtained (29 mL) is rounded to two significant figures. When multiplying or dividing, the amount of significant figures in the final answer is always the least amount of significant figures in one of the values.

Below are the significant figure rules:

Nonzero digits will always be significant (eg. 54 --> 2 significant figures)

Zeroes at the beginning of a number will never be significant (eg. 0.1 --> 1 significant figure)

Zeroes between two nonzero digits will always be significant (eg. 504 --> 3 significant figures)

Zeroes following a number will always be significant if the number contains a decimal point (eg. 40.0 --> 3 significant figures)

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By formula; density= mass/volume; d=m/V

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