Step-by-step explanation:
We have a gas sample of carbon dioxide and we know its volume, the pressure and the temperature. We can find the number of moles of that sample using the ideal gas law.
P * V = n * R * T
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas law and T is the temperature.
R = 0.082 atm*L/(mol*K)
Since R is in atm*L/(mol*K) we have to convert the volume from mL to L, the temperature from °C to K and the pressure from torr to atm.
1000 mL = 1 L
V = 26 mL = 26 mL * 1 L/(1000 mL)
V = 0.026 L
760 torr = 1 atm
P = 623 torr = 623 torr * 1 atm/(760 torr)
P = 0.820 atm
T = (273.15 + 11 ) K
T = 284.15 K
Now we can replace these values in the formula and solve it for n to find the number of moles that are present in the sample.
P * V = n * R * T
n = P * V/(R * T)
n = 0.820 atm * 0.026 L/(0.082 atm*L/(mol*K) * 284.15 K)
n = 0.000915 mol
Finally we can convert the moles of the sample into grams using the molar mass of carbon dioxide.
molar mass of C = 12.01 g/mol
molar mass of O = 16.00 g/mol
molar mass of CO₂ = 1 * 12.01 g/mol + 2 * 16.00 g/mol
molar mass of CO₂ = 44.01 g/mol
mass of CO₂ = 0.000915 mol * 44.01 g/mo
mass of CO₂ = 0.040 g
Answer: There are 0.040 g of carbon dioxide in the sample.