What is the mass of one mole of carbon dioxide, CO2? Round your answer to 2 places past the decimal. 28.0144.0044.01

The mass of one mole of carbon dioxide, rounded to two decimal places is 44.01g.

Expert answered|OneRepublic|Points 655|

Question

Asked 2/28/2012 1:39:57 PM

Updated 2/28/2012 1:54:05 PM

1 Answer/Comment

This conversation has been flagged as incorrect.

Rating

3

The mass of one mole of carbon dioxide, rounded to two decimal places is 44.01g.

Added 2/28/2012 1:54:05 PM

This answer has been added to the Weegy Knowledgebase

A 25-liter sample of steam at 100°C and 1.0 atm is cooled to 25°C and expanded until the pressure is 19.71 mmHg. If no water condenses, calculate the final volume of the water vapor.
770 L
240 L
1.3 x 10-3 L
1.0 L
**Weegy:** A) 770 L
It will condense, because steam becomes liquid water below 100°C. **User:** A diesel engine's piston compresses 16 cm3 of fuel-air mixture into 1 cm3. The pressure changes from 1 atmosphere to 48 atmospheres. If the initial temperature of the gas was 305 K, what was the final temperature?
Note: As long as the units for pressure and volume are the same on both sides of the equation, they will cancel. Temperature, however, must be in units of kelvin. Be sure to use the proper number of significant figures.
915 K
1.09 x 10-3 K
900 K
100 K
**Weegy:** 100 K T = 305 K[(1 atm)/(48 atm)][(16 cm^3)/(1 cm^3)] (More)

Question

Expert Answered

Asked 2/27/2012 5:21:42 PM

0 Answers/Comments

Which of these expressions are correct variations of the Combined Gas Law?
P1V1T2 = P2V2T1
both
**Weegy:** P1V1T2 = P2V2T1 both
both correct (More)

Question

Expert Answered

Asked 2/27/2012 6:01:43 PM

0 Answers/Comments

The mathematical formula for Boyle's Law is:
P/V = k
P1/V1= P2V2
P/T = k
P1V1 = k
PT = k
**Weegy:** The mathematical equation for Boyle's law is PV = k or you could say P1V1=P2V2.
P IS the pressure of the system.
V is the volume of the gas.
k is a constant value representative of the pressure and volume of the system. [
**It just states that pressure and volume are inversely proportional when temperature is held constant (does not change). In other words, as volume increases pressure decreases and vice-versa (when temperature is constant).**
Also, an easy way to remember all of the laws (Boyle's, Charles', and Gay-Lussac's) is to remember one equation: The Ideal Gas Equation, which happens to be PV=nRT. P=pressure, V=volume, n=number of moles, R=constant (varies with certain units, for example, when using torrs or mm Hg it would equal 62.4), and T=temperature. You can make basic assumptions from this equation, for example, you know that when temperature is held constant that if pressure increases volume must decrease (which happens to be Boyle's Law).
] **User:** A man drove his car through the Nevada desert one day when the temperature was over 100°F. When he started the trip, the gas station attendant found the tire to be 32 lb/in². When he filled up with gas after crossing the desert, an attendant found the tire pressure to be 38 lb/in². The best explanation for the increase in tire pressure is:
The road wear on the tire caused a decrease in volume, therefore an increase in tire pressure.
The temperature in the tire increased, causing an increased tire pressure.
The hot temperature caused the springs to expand, which allowed more weight to ride on the tires, thus causing more pressure inside.
The measurements of the pressure were inaccurate. The added weight of the gas caused the extra pressure in the tires.
(More)

Question

Expert Answered

Asked 2/28/2012 1:00:04 PM

0 Answers/Comments

What will be the new volume of a 250 mL sample of gas at 300 K and 1 atm if heated to 350 K at 1 atm?
**Weegy:** 291.67 ml **User:** Determine which law is appropriate for solving the following problem.
What volume will 1.56 liters of a gas at 27°C and 745 mmHg of pressure occupy at 100°C and 700 mmHg of pressure?
**Weegy:** Ideal Gas Law **User:** Determine which law is appropriate for solving the following problem.
What temperature will 215 mL of a gas at 20°C and 1 atm pressure attain when it is subject to 1.5 atm of pressure?
Law used: Boyle's LawCharles' LawCombined Gas Law
**Weegy:** Combined Gas Law **User:** Determine which law is appropriate for solving the following problem.
When the volume changes from 63.5 mL to 69.2 mL, what is the final pressure if the initial pressure was 735 mmHg pressure?
Law used: Boyle's LawCharles' LawCombined Gas Law
**Weegy:** Boyle's Law (More)

Question

Expert Answered

Asked 2/28/2012 12:46:57 PM

0 Answers/Comments

A tire has a pressure of 780 mmHg at 27°C. If the tire is heated to 47°C on hot pavement, the new pressure will be:
310 mmHg
280 mmHg
830 mmHg
590 mmHg
none of these
**Weegy:** 830 mmHg **User:** A 1.50-liter sample of dry air in a cylinder exerts a pressure of 3.0 atmospheres at a temperature of 25°C. Without change in temperature, a piston is moved in the cylinder until the pressure in the cylinder is reduced to 1.0 atmosphere. What is the volume of the gas? (Be sure to use the correct number of significant figures.)
0.22 L
0.50 L
2.0 L
4.5 L
**Weegy:** Answer is 4.5 L (More)

Question

Expert Answered

Asked 2/28/2012 1:11:06 PM

0 Answers/Comments

26,802,179 questions answered

There are no comments.