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3 years ago

Suppose a 5.00 l sample of o2 at a given temperature and pressure contains 1.08

1 answer:

5 0

Missing question: A 5.00 L sample of O2 at a given temperature and pressure contains a 1.08x10^23 molecules. How many molecules would be contained in each of the following at the same temperature and pressure? 
a) 5.00 L H2.
b) 5.00 L CO2.
Use Avogadro's Law: The Volume Amount Law: equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. Because hydrogen and carbon(IV) oxide are gases, number of molecules are the same as number of oxygen molecules, so:
a) N(H₂) = 1.08·10²³.
b) N(CO₂) = 1.08·10²³

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The pOH of a solution of KOH is 11.30. What is the [H*] for this solution?

Sloan [31]

Answer: The concentration of hydrogen ions for this solution is $1.99 \times 10^{-3}$ .

Explanation:

Given: pOH = 11.30

The relation between pH and pOH is as follows.

pH + pOH = 14

pH + 11.30 = 14

pH = 14 - 11.30

= 2.7

Also, pH is the negative logarithm of concentration of hydrogen ions.

$pH = - log [H^{+}]$

Substitute the values into above formula as follows.

$pH = -log [H^{+}]\\2.7 = -log [H^{+}]\\conc. of H^{+} = 1.99 \times 10^{-3}$

Thus, we can conclude that the concentration of hydrogen ions for this solution is $1.99 \times 10^{-3}$ .

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3 years ago

How do radiography and sonography compare?

lara [203]

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(Credits to google)

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4 years ago

Read 2 more answers

Compared to the normal freezing point and boiling point of water, a 1-molar solution of sugar in water will have a

marysya [2.9K]

Answer :

Boiling point of the sugar solution will be higher than that of water's boling point.
Freezing point of the sugar solution will be lower than that of water's freezing point.

Explanation:

Boiling point of a liquid is defined as temperature at which vapor pressure of liquid becomes equal to the atmospheric pressure.

Boiling point of solution is always higher than that of the pure solvent

Vapor pressure increases with increase in temperature which means sugar solution will be heated more to make vapor pressure equal to atmospheric pressure.

Freezing point is defined as temperature at which solid and liquid phase are at equilibrium or temperature at which vapor pressure of liquid becomes equal to the vapor pressure in its solid phase.

Freezing point of solution is always lower than that of the pure solvent.

Lower the temperature, lower will be the vapor pressure which sugar solution solution will get freeze at lower temperature than that of the water.

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3 years ago

Picture of gas laws question below:

Vera_Pavlovna [14]

Volume of the tank is 5.5 litres.

Explanation:

mass of the CO2 is given 8.6 grams

Pressure of the gas is 89 Kilopascal which is 0.8762 atm

Temperature of the gas is 29 degrees ( 0 degrees +273.5= K) so (29+273)

R = gas constant 0.0821 liter atmosphere per kelvin)

FROM THE IDEAL GAS LAW

PV=nRT ( P Pressure, V Volume, n is number of moles of gas, R gas constant, Temperature in Kelvin)

no of moles = mass/atomic mass

= 8.6/44

= 0.195 moles

now putting the values in equation

V=nRT/P

= 0.195*0.0821*302/ 0.8762

= 5.5 litres.

As the carbon dioxide gas occupies the volume os the tank hence volume of tank is 5.5 litres.

4 0

3 years ago

how much water should be added to 1 gallon of pure antifreeze to obtain a solution that is 60% antifreeze?

antoniya [11.8K]

1 gallon of antifreeze = 60% of mixture. Total mixture:
Vm = 1/0.6
= 1.67 gallons

Volume of water = total vol - antifreeze vol
= 1.67 - 1
= 0.67 gallon of water

7 0

3 years ago