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ser-zykov [4K]
2 years ago
13

On a cool, rainy day, the barometric pressure is 698 mmHg. Calculate the barometric pressure in centimeters of water (cmH2O). De

nsity of Hg = 13.5 g/mL; d of H2O = 1.00 g/mL.
Chemistry
1 answer:
lesantik [10]2 years ago
7 0

Answer:

Barometric pressure is 942.3 cm of column of water.

Explanation:

We can measure barometric pressure by measuring the height h of a column of fluid (this column of fluid exerts the same pressure as the column of air of which we are measuring pressure) using the following formula:

P = \rho*g*h\\

Where ρ is the density of the fluid used and g the acceleration of gravity.

Knowing that both the column of mercury (to match units, we know that 698 mmHg are the same as 69.8 cmHg) and the column of water are representing the same pressure, we can match expressions and find h for the column of water:

\rho_{Hg} *g*h_{Hg} =\rho_{Water} *g*h_{Water}\\ \\h_{Water}=\frac{rho_{Hg} *g*h_{Hg}}{\rho_{Water} *g} = \frac{13.5g/mL *9.8m/s^{2} *69.8cm}{1g/mL *9.8m/s^{2}}=942.3 cmH_{2}O

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viva [34]

Answer:

Your answer would be C.

Explanation:

Gamma radiation, unlike alpha or beta, does not consist of any particles, instead consisting of a photon of energy being emitted from an unstable nucleus. Having no mass or charge, gamma radiation can travel much farther through air than alpha or beta, losing (on average) half its energy for every 500 feet.

4 0
3 years ago
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Why would you add boiling chips/stones to a solution that is to be refluxed? when should you add them?
anygoal [31]
Answer: Boiling chips provide surfaces on which bubbles can form as the liquid boils.

Hope this helps!
6 0
3 years ago
An ideal gas occupies a volume V at an absolute temperature T. If the volume is halved and the pressure kept constant, what will
Kruka [31]

Answer:

It will be halve of T

Explanation:

V1 = V

T1 = T

V2 = ½V

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V1/T1 = V2/T2

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6 0
3 years ago
How many grams of octane (C8H18) must be burned to produce 300.0g of CO2?
nika2105 [10]

Answer:

m_{C_8H_{18}}=85.67gC_8H_{18}

Explanation:

Hello there!

In this case, according to the given combustion reaction of octane, it is possible for us to perform the stoichiometric method in order to calculate the mass of octane that is required to consume 300.0 g of oxygen by considering the 2:25 mole ratio, and the molar masses of 114.22 g/mol and 32.00 g/mol respectively:

m_{C_8H_{18}}=300.0gO_2*\frac{1molO_2}{32.00gO_2}*\frac{2molC_8H_{18}}{25molO_2}*\frac{114.22gC_8H_{18}}{1molC_8H_{18}}   \\\\m_{C_8H_{18}}=85.67gC_8H_{18}

Regards!

6 0
3 years ago
In the laboratory you dissolve 13.9 g of potassium phosphatein a volumetric flask and add water to a total volume of 250mL.
tensa zangetsu [6.8K]

Answer:

Molarity of the solution? 0,262 M.

Concentration of the potassium cation? 0,786 M.

Concentration of the phosphate anion? 0,262 M.

Explanation:

Potassium phosphate (K₃PO₄; 212,27 g/mol) dissolves in water thus:

K₃PO₄ → 3 K⁺ + PO₄³⁻ <em>(1)</em>

Molarity is an unit of chemical concentration given in moles of solute (K₃PO₄) per liters of solution.

There are 250 mL of solution≡0,25 L

The moles of K₃PO₄ are:

13,9 g of K₃PO₄ ×\frac{1mol}{212,27 g} = 0,0655 moles of K₃PO₄

The molarity of the solution is:

\frac{0,0655 moles}{0,25L} = 0,262 M

In (1) you can see that 1 mole of K₃PO₄ produces 3 moles of potassium cation. The moles of potassium cation are:

0,0655 moles×3 = 0,1965 moles

The concentration is:

\frac{0,1965 moles}{0,25L} = 0,786 M

The moles of K₃PO₄ are the same than moles of PO₄³⁻, thus, concentration of phosphate anion is the same than concentration of K₃PO₄. 0,262 M

I hope it helps!

4 0
3 years ago
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