which of the following gasses will have the largest volume ( all volumes are measured at the same temperature and pressure)
A) 16g of CH4
B) 34g of NH3
C) 44g of co2
D) 64g of SO2
i think the answer is C am i right
You may or may not be right. How did you get your answer? That is the important part.
i found the gram formula mass for each gas and took it away from the gram given in the example
Close but no cigar.
You find the gram formula mass, which is
16 for CH4
17 for NH3
44 for CO2
64 for SO2.
So you have 1 mole CH4
2 moles NH3
1 mole CO2
1 mole for SO2.
Now which will occupy the most volume at the same P and T.
You may want to use
PV = nRT
You know P is the same, R is the same, T is the same. So the highest V is for the xxxxx n.
To determine which gas will have the largest volume, we need to compare the amounts of each gas using their molar masses.
First, let's calculate the number of moles for each gas using the formula:
Number of moles = Mass of gas / Molar mass of gas
A) CH4:
Number of moles = 16g / 16.04g/mol (molar mass of CH4) ≈ 0.997 moles
B) NH3:
Number of moles = 34g / 17.03g/mol (molar mass of NH3) ≈ 1.996 moles
C) CO2:
Number of moles = 44g / 44.01g/mol (molar mass of CO2) ≈ 0.999 moles
D) SO2:
Number of moles = 64g / 64.06g/mol (molar mass of SO2) ≈ 0.999 moles
Next, we consider the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles when temperature and pressure are constant:
V ∝ n (volume is proportional to moles)
Since the number of moles is closest to 1 (which is more significant than the actual value), it suggests that the gas with the highest number of moles will have the largest volume.
Therefore, in this case, the correct answer is indeed C) 44g of CO2, as it has the highest number of moles, resulting in the largest volume.