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3 years ago

_________________________________ data are related to descriptive information that is expressed as a

2 answers:

4 0

The answer would be quantity date for both of them message me if you don’t understand I would be happy to answer any question.

ICE Princess25 [194]3 years ago

3 0

Answer:

qualitative data

and

quanitative data

Explanation:

hope this helps and PLZ brainliest thank you

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According to Newton's 1st law of motion, what is required to make an object slow down?

attashe74 [19]

Newton’s first law state that an object in motion stays in motion unless acted upon force so the answer would be RESISTANCE

7 0

3 years ago

Read 2 more answers

A sample of CaCO3 (molar mass 100. g) was reported as being 30. percent Ca. Assuming no calcium was present in any impurities, c

natka813 [3]

Answer:

Approximately 75%.

Explanation:

Look up the relative atomic mass of Ca on a modern periodic table:

Ca: 40.078.

There are one mole of Ca atoms in each mole of CaCO₃ formula unit.

The mass of one mole of CaCO₃ is the same as the molar mass of this compound: $\rm 100\; g$ .
The mass of one mole of Ca atoms is (numerically) the same as the relative atomic mass of this element: $\rm 40.078\; g$ .

Calculate the mass ratio of Ca in a pure sample of CaCO₃:

$\displaystyle \frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)} = \frac{40.078}{100} \approx \frac{2}{5}$ .

Let the mass of the sample be 100 g. This sample of CaCO₃ contains 30% Ca by mass. In that 100 grams of this sample, there would be $\rm 30 \% \times 100\; g = 30\; g$ of Ca atoms. Assuming that the impurity does not contain any Ca. In other words, all these Ca atoms belong to CaCO₃. Apply the ratio $\displaystyle \frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)} \approx \frac{2}{5}$ :

$\begin{aligned} m\left(\mathrm{CaCO_3}\right) &= m(\mathrm{Ca})\left/\frac{m(\mathrm{Ca})}{m\left(\mathrm{CaCO_3}\right)}\right. \cr &\approx 30\; \rm g \left/ \frac{2}{5}\right. \cr &= 75\; \rm g \end{aligned}$ .

In other words, by these assumptions, 100 grams of this sample would contain 75 grams of CaCO₃. The percentage mass of CaCO₃ in this sample would thus be equal to:

$\displaystyle 100\%\times \frac{m\left(\mathrm{CaCO_3}\right)}{m(\text{sample})} = \frac{75}{100} = 75\%$ .

3 0

2 years ago

To begin the experiment, a bomb calorimeter is filled with 1.11 g CH4 and an excess of oxygen. The heat capacity of the calorime

Flura [38]

There are several information's already given in the question. Based on those information's the answer can be easily determined.

M = <span>1.11 g CH4
C = </span>4.319 kJ g C⋅°
∆T = 35.65 - 24.85 degree centigrade
= 10.8 degree centigrade.
Then
∆H =−M ⋅ C ⋅∆T
= - 1.11 * 4.319 * 10.8
= - 51.776 kJ/<span>mol

I hope the procedure is clear enough for you to understand.</span>

6 0

2 years ago

PLEASE HELP ME The pH scale for acids and bases ranges from _____.

inysia [295]

The pH scale for acids and bases ranges from 1 - 14. The answer is letter C. The rest of the choices do not answered the question above. There are quite a few relationships between [H+] and [OH−] ions. And because there is a large range of number between 10 to 10-15 M, the pH is used. pH = -log[H+] and pOH = -log[OH−]. In aqueous solutions, [H+ ][OH- ] = 10-14. From here we can derive the values of each concentration.

-log[H+ ] + -log[OH- ] = -log[10-14]

pH + pOH = 14

So pH = 14 – pOH and pOH = 14 –

It would be B.

7 0

3 years ago

Why is soap so effective at killing microorganisms?

IceJOKER [234]

Answer:

— Washing with soap and water is an effective way to destroy and dislodge many microbes

Explanation:

Soap actually kill germs on our hands, it breaks them up and removes them
.But soap molecules have two different ends to them.
One end is attracted to water molecules – this is called hydrophilic
– and the other end loves oil and fat molecules – this is called hydrophobic.
Soap is able to bind to the oils on our hands, and then mix with the water to wash all the germs away.

4 0

2 years ago