Which of the following is the best thermal insulator to reduce the transfer of

Determine the specific heat of a 70 g sample of material that absorbed 96 J as it was heated from 293 K to 313 K

Damm [24]

This problem is providing us with the mass (70 g), absorbed heat (96 J) and initial and final temperatures (293 K and 313 K, respectively) so the specific heat of the material is required and found to be 0.0686 J/(g*K) as shown below:

<h3>Calorimetry:</h3>

In chemistry, we can go over calorimetry by writing the following relationship among heat, mass, specific heat and temperature change:

$Q=mC(T_f-T_i)$

Thus, one can get the specific heat by solving for C in the previous equation:

$C=\frac{Q}{m(T_f-T_i)}$

Hence, we can plug in the given data to obtain:

$C=\frac{96J}{70g(313K-293K)}\\ \\C=0.0686\frac{J}{g*K}$

Learn more about calorimetry: brainly.com/question/1407669

5 0

2 years ago

Why water is able to stick to the side of a glass

Snezhnost [94]

Answer:

Water uses adhesive forces that allow it to stick to certain surfaces such as glass.

Explanation:

When the angle between vertical direction and the glass wall is small, surface tension is stronger and the component of gravity perpendicular to the glass wall is small. The result of this causes water to stick to the side of a glass.

Hope this helps!

3 0

3 years ago

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URGENT PLEASE HELP!!

Orlov [11]

Answer:

Liters per second is 0.2 LPS

Liters per hour is 720

Explanation:

Divide the litres by the time, than multiply the time of an hour (in seconds) and than multiply the lps by time of an hour in seconds.

3 0

3 years ago

What is the empirical formula of an oxide of nitrogen containing 63.61% by mass of nitrogen and 36.69% by mass of oxygen?

ioda

N₂O is the empirical formula of an oxide of nitrogen containing 63.61% by mass of nitrogen and 36.69% by mass of oxygen.

Empirical formula can be calculated by

Suppose we have 100 g of the substance. That indicates that it has 36.69 grams of oxygen and 63.61 grams of nitrogen.

Masses transformed into moles:

Formula used

Given mass/ Molar mass

14.01 g contains 1 mol of N

So 63.61 g of N contains moles is equals to

(1 mol N / 14.01 g N) 63.61 g N = 4.540 mol N

Similarly

16 g of O contains 1 mole of O

36.69 g of O contains moles is equals to

(1 mol O / 16.00 g O) 36.69 g O = 2.293 mol O

Divide by the smallest to normalize:

4.540 / 2.293 = 1.980 mol N

2.293 / 2.293 = 1.000 mol O

Therefore, there are roughly twice as many N as O atoms. N2O is the empirical formula as a result.

Ratio is basically 2:1

Hence, N₂O is the empirical formula of an oxide of nitrogen

Learn more about Empirical Formula here brainly.com/question/27873410

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7 0

2 years ago

Which is the best description of a molecule?

Archy [21]

A. molecule is created when two of more atoms are chemically bonded .

3 0

4 years ago

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