Which of the following gases occupy the smallest volume at STP?
a
4.032 g H2
b
1.000 mol of carbon dioxide
c
6.022 × 1023 molecules of O2
d
35.45 g Cl2
1.000
To determine which gas occupies the smallest volume at STP (Standard Temperature and Pressure), we need to compare the number of moles of each gas.
First, let's convert the given information into moles for each gas:
a) 4.032 g of H2:
To convert grams to moles, we need to divide the given mass by the molar mass of H2. The molar mass of H2 is 2.02 g/mol.
4.032 g H2 / 2.02 g/mol = 1.998 mol H2
b) 1.000 mol of carbon dioxide (CO2):
No conversion is needed here since the given quantity is already in moles.
c) 6.022 × 10^23 molecules of O2:
To convert molecules to moles, we need to divide the given quantity by Avogadro's number, which is approximately 6.022 × 10^23 molecules per mole.
6.022 × 10^23 molecules / 6.022 × 10^23 molecules/mol = 1 mol O2
d) 35.45 g Cl2:
To convert grams to moles, we need to divide the given mass by the molar mass of Cl2. The molar mass of Cl2 is 70.90 g/mol.
35.45 g Cl2 / 70.90 g/mol = 0.499 mol Cl2
Now, looking at the moles of each gas:
a) 1.998 mol H2
b) 1.000 mol CO2
c) 1.000 mol O2
d) 0.499 mol Cl2
Since the number of moles of each gas is approximately the same, we can conclude that all the gases occupy a similar volume at STP.