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Dmitry [639]
2 years ago
13

Explain why pure water is a compound, but water from a fountain is not.

Chemistry
1 answer:
myrzilka [38]2 years ago
7 0
I’m distilled water all of the dissolved substances mixed in water have been removed by evaporation.
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Relative to protons, electrons have:
saw5 [17]

Answer:

<u><em>(B.) a significantly lower mass that protons</em></u>

Explanation:

The mass (in g) of an electron is 9.11 ×10^{-28}g, which is significantly lower than the mass of protons and neutrons which are approximately the same. They are extremely small (equal to 0 amu), contributing nothing to the overall mass of the atom.

The nucleus has a mass of 1 amu and is positively charged.

6 0
3 years ago
Which statement applies to electronegativity?
EastWind [94]
I believe the answer would be A. Electronegativity increases across a period.
6 0
3 years ago
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A substance that contains only one type of particle is an __________​
Dvinal [7]

the answer is a chemical element

7 0
3 years ago
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What is the equation for the average?
s2008m [1.1K]

Explanation:

The equation for the average is: (sum of all data values/ (total number of data values)

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3 years ago
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I need help solving this!
zmey [24]

Answer: Moles of hydrogen required are 4.57 moles to make 146.6 grams of methane, CH_{4}.

Explanation:

Given: Mass of methane = 146.6 g

As moles is the mass of a substance divided by its molar mass. So, moles of methane (molar mass = 16.04 g/mol) are calculated as follows.

Moles = \frac{mass}{molar mass}\\= \frac{146.6 g}{16.04 g/mol}\\= 9.14 mol

The given reaction equation is as follows.

C + 2H_{2} \rightarrow CH_{4}

This shows that 2 moles of hydrogen gives 1 mole of methane. Hence, moles of hydrogen required to form 9.14 moles of methane is as follows.

Moles of H_{2} = \frac{9.14}{2}\\= 4.57 mol

Thus, we can conclude that moles of hydrogen required are 4.57 moles to make 146.6 grams of methane, CH_{4}.

5 0
3 years ago
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