125k views
2 votes
What is the mass of 29.3 L of carbon monoxide at STP?

hey guys.. show. work.. i have no idea whats going on

User Tokhi
by
8.2k points

1 Answer

3 votes

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.

User Fishdrowned
by
7.3k points

No related questions found