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Mekhanik [1.2K]
2 years ago
15

4

Chemistry
2 answers:
saveliy_v [14]2 years ago
7 0

Answer:

Is A- Carbon Dioxide

Explanation:

other air pollutants collect in the atmosphere and absorb sunlight and solar radiation that have bounced off the earth's surface.

Llana [10]2 years ago
3 0

Answer:Carbon dioxide would be your best choice.

Explanation:

You might be interested in
Amoxicillin Suspension 125 mg/ 5 ml is 125 mg of Amoxicillin per 5 ml of suspension is an example of weight to ________.
kkurt [141]

Answer : Amoxicillin Suspension 125 mg/ 5 ml is 125 mg of Amoxicillin per 5 ml of suspension is an example of weight to volume.

Explanation :

Weight by volume (w/v) means that the mass of solute present in 100 mL volume of solution.

Weight by weight (w/w) means that the mass of solute present in 100 gram of solution.

Volume by volume (v/v) means that the volume of solute present in 100 mL volume of solution.

As per question, amoxicillin suspension is, 125 mg/ 5 ml that means 125 mg of Amoxicillin present in 5 mL of suspension. So, it is an example of weight to volume.

Hence, it is an example of weight to volume.

8 0
3 years ago
What volume of nitrogen gas is equal too 3.42x10^22 molecules of this substance
Bas_tet [7]

if i am correct the volume of nitrogen gas has to equal to molecules density, making the substance 1.27 liters :)

8 0
2 years ago
At standard temperature and pressure, what volume does 0.5 mol of CO2 occupyAt standard temperature and pressure, what volume do
Zigmanuir [339]
<span>C. 11.2 L There are several different ways to solve this problem. You can look up the density of CO2 at STP and work from there with the molar mass of CO2, but the easiest is to assume that CO2 is an ideal gas and use the ideal gas properties. The key property is that a mole of an idea gas occupies 22.413962 liters. And since you have 0.5 moles, the gas you have will occupy half the volume which is 22.413962 * 0.5 = 11.20698 liters. And of the available choices, option "C. 11.2 L" is the closest match. Note: The figure of 22.413962 l/mole is using the pre 1982 definition of STP which is a temperature of 273.15 K and a pressure of 1 atmosphere (1.01325 x 10^5 pascals). Since 1982, the definition of STP has changed to a temperature of 273.15 K and a pressure of exactly 10^5 pascals. Because of this lower pressure, one mole of an ideal gas will have the higher volume of 22.710947 liters instead of the older value of 22.413962 liters.</span>
4 0
3 years ago
PLEASE HELP ME!!!
irina [24]

that's the answer I think

6 0
2 years ago
Read 2 more answers
At a given temperature the vapor pressures of hexane and octane are 183 mmhg and 59.2 mmhg, respectively. Calculate the total va
Bas_tet [7]

Total vapor pressure can be calculated using partial vapor pressures and mole fraction as follows:

P=X_{A}P_{A}+X_{B}P_{B}

Here, X_{A} is mole fraction of A, X_{B} is mole fraction of B, P_{A} is partial pressure of A and P_{B} is partial pressure of B.

The mole fraction of A and B are related to each other as follows:

X_{A}+X_{B}=1

In this problem, A is hexane and B is octane, mole fraction of hexane is given 0.580 thus, mole fraction of octane can be calculated as follows:

X_{octane}=1-X_{hexane}=1-0.58=0.42

Partial pressure of hexane and octane is given 183 mmHg and 59.2 mmHg respectively.

Now, vapor pressure can be calculated as follows:

P=X_{hexane}P_{hexane}+X_{octane}P_{octane}

Putting the values,

P=(0.580)(183 mmHg)+(0.420)(59.2 mmHg)=131 mmHg

Therefore, total vapor pressure over the solution of hexane and octane is 131 mmHg.

4 0
3 years ago
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