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kodGreya [7K]
3 years ago
14

The Groups 1 and 2 on the periodic table contain what atom type?

Chemistry
2 answers:
Bumek [7]3 years ago
8 0
Non metals
and metals
coldgirl [10]3 years ago
3 0
Metals and also nonmetals
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The answer is <span>Potassium cyanide</span>
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If 32.3 grams of KCl are dissolved in 192 grams of water, what is the concentration of the solution in percent by mass?
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The concentration is 0.168 g/ml
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A sample of helium gas has a volume of 2.0 L at a pressure of 4.0 atm. What is the volume of gas at 380 mmHg
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From equation;
P1V1=P2V2
V2=P1V1÷P2
since P2=380mmHg
now;1atm=760mmHg
how about 380mmHg is equal to how many atm?
380×1÷760=0.5atm
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back from equation;
P1V1=P2V2
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3 years ago
The Doppler. Effect indicates that the universe is expanding because
GalinKa [24]

Answer : The correct answer is option C.

Explanation:

Astronomers have observed that light from the distant object in the universe is shifted towards the frequency of red color which indicates that those object are receding or moving away from the planet earth.This phenomena was termed as Red shift .Same thing goes for galaxies which are very far away from the planet earth.

Where as if galaxies were moving towards the the planet earth their light would have shifted toward the frequency of blue color termed as blue shift.

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A hypothetical element has an atomic weight of 48.68 amu. It consists of three isotopes having masses of 47.00 amu, 48.00 amu, a
Morgarella [4.7K]

Answer : The percent abundance of the heaviest isotope is, 78 %

Explanation :

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i

As we are given that,

Average atomic mass = 48.68 amu

Mass of heaviest-weight isotope = 49.00 amu

Let the percentage abundance of heaviest-weight isotope = x %

Fractional abundance of heaviest-weight isotope = \frac{x}{100}

Mass of lightest-weight isotope = 47.00 amu

Percentage abundance of lightest-weight isotope = 10 %

Fractional abundance of lightest-weight isotope = \frac{10}{100}

Mass of middle-weight isotope = 48.00 amu

Percentage abundance of middle-weight isotope = [100 - (x + 10)] %  = (90 - x) %

Fractional abundance of middle-weight isotope = \frac{(90-x)}{100}

Now put all the given values in above formula, we get:

48.68=[(47.0\times \frac{10}{100})+(48.0\times \frac{(90-x)}{100})+(49.0\times \frac{x}{100})]

x=78\%

Therefore, the percent abundance of the heaviest isotope is, 78 %

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3 years ago
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