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3 years ago

Will give brainliest to the correct answer

Chemistry

2 answers:

enyata [817]3 years ago

8 0

Answer:

Offsprings are more rapidly reproduced

Explanation:

Pavel [41]3 years ago

3 0

Offspring are more rapidly reproduced

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A class is 47 min how many seconds is this ?

Sonbull [250]

Answer: 2820 seconds

1 minute = 60 seconds

Multiply the value times 60

47×60=2820

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3 years ago

What is the average mass of a single sulfur atom in grams?

Nostrana [21]

32.066 atomic mass units.

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3 years ago

The partial pressure of CO2 gas in a bottle of carbonated water is 4.60 atm at 25 ºC. How much CO2 gas (in g) will be released f

frutty [35]

If the partial pressure of CO₂ in a bottle of carbonated water decreases from 4.60 atm to 1.28 atm, the mass of CO₂ released is 0.265 g.

The partial pressure of CO₂ gas in a bottle of carbonated water is 4.60 atm at 25 ºC. We can calculate the concentration of CO₂ using Henry's law.

$C = k \times P = \frac{1.65 \times 10^{-3} M }{atm} \times 4.60 atm = 7.59 \times 10^{-3} M$

We can calculate the mass of CO₂ in 1.1 L considering its molar mass is 44.01 g/mol.

$\frac{7.59 \times 10^{-3} mol}{L} \times 1.1 L \times \frac{44.01 g}{mol} = 0.367 g$

Now, we will repeat the same procedure for a partial pressure of 1.28 atm.

$C = k \times P = \frac{1.65 \times 10^{-3} M }{atm} \times 1.28 atm = 2.11 \times 10^{-3} M$

$\frac{2.11 \times 10^{-3} mol}{L} \times 1.1 L \times \frac{44.01 g}{mol} = 0.102 g$

The mass of CO₂ released will be equal to the difference in the masses at the different pressures.

$m = 0.367 g - 0.102 g = 0.265 g$

If the partial pressure of CO₂ in a bottle of carbonated water decreases from 4.60 atm to 1.28 atm, the mass of CO₂ released is 0.265 g.

Learn more: brainly.com/question/18987224

<em>The partial pressure of CO₂ gas in a bottle of carbonated water is 4.60 atm at 25 ºC. How much CO₂ gas (in g) will be released from 1.1 L of the carbonated water when the partial pressure of CO2 is lowered to 1.28 atm? At 25 ºC, the Henry’s law constant for CO₂ dissolved in water is 1.65 x 10⁻³ M/atm, and the density of water is 1.0 g/cm³.</em>

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2 years ago

A chemist must dilute 34.3mL of 1.72mM aqueous calcium sulfate solution until the concentration falls to 1.00mM. He'll do this b

EastWind [94]

Answer:

58.9mL

Explanation:

Given parameters:

Initial volume = 34.3mL = 0.0343dm³

Initial concentration = 1.72mM = 1.72 x 10⁻³moldm⁻³

Final concentration = 1.00mM = 1 x 10⁻³ moldm⁻³

Unknown:

Final volume =?

Solution:

Often times, the concentration of a standard solution may have to be diluted to a lower one by adding distilled water. To find the find the final volume, we must recognize that the number of moles of the substance in initial and final solutions are the same.

Therefore;

C₁V₁ = C₂V₂

where C and V are concentration and 1 and 2 are initial and final states.

now input the variables;

1.72 x 10⁻³ x 0.0343 = 1 x 10⁻³ x V₂

V₂ = 0.0589dm³ = 58.9mL

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3 years ago

Which of the following is a pure substance

sergij07 [2.7K]

What is the following

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3 years ago