Answer:
33.67g
Step-by-step explanation:
To calculate the mass of carbon monoxide, we can use the ideal gas law, which relates the pressure, volume, number of moles, and temperature of a gas:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
At STP (standard temperature and pressure), the pressure is 1 atm and the temperature is 273.15 K. The ideal gas constant is R = 0.08206 L atm/(mol K).
To find the number of moles of carbon monoxide in 29.3 L at STP, we can rearrange the ideal gas law to solve for n:
n = PV/(RT)
n = (1 atm)(29.3 L)/(0.08206 L atm/(mol K) * 273.15 K)
n = 1.203 mol
The molar mass of carbon monoxide (CO) is 28.01 g/mol. Therefore, the mass of 1.203 mol of CO is:
mass = n * molar mass
mass = 1.203 mol * 28.01 g/mol
mass = 33.67 g
Therefore, the mass of 29.3 L of carbon monoxide at STP is approximately 33.67 grams.