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

Chemistry

2 answers:

wariber [46]3 years ago

5 0

CO2 has one mole at the mass of 44.01g/mol

Whitepunk [10]3 years ago

5 0

Answer:

$44~\frac{g}{mol}$

Explanation:

If we want to calculate the molar mass of this compound we have to find the atomic masses of each atom, in this case:

Oxygen = $16~\frac{g}{mol}$

Carbon= $12~\frac{g}{mol}$

Then we have to multiply the atomic mass by the number of atoms in the compound, so:

$(16*2)+(12*1)=~44\frac{g}{mol}$

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How many grams of O2 are present in 44.1 L of O2 at STP?

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Taking into accoun the STP conditions and the ideal gas law, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.

First of all, the STP conditions refer to the standard temperature and pressure, where the values used are: pressure at 1 atmosphere and temperature at 0°C. These values are reference values for gases.

On the other side, the pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

P is the gas pressure.
V is the volume that occupies.
T is its temperature.
R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
n is the number of moles of the gas.

Then, in this case:

P= 1 atm
V= 44.1 L
n= ?
R= 0.082 $\frac{atmL}{molK}$
T= 0°C =273 K

Replacing in the expression for the ideal gas law:

1 atm× 44.1 L= n× 0.082 $\frac{atmL}{molK}$ × 273 K

Solving:

$n=\frac{1 atm x44.1 L}{0.082\frac{atmL}{molK}x273K}$

n=1.97 moles

Being the molar mass of O₂, that is, the mass of one mole of the compound, 32 g/mole, the amount of mass that 1.97 moles contains can be calculated as:

$1.97 molesx\frac{32 g}{1 mole}$ = 63.04 g ≈ 63 g