How many grams of CO2 are contained in 550 mL of the gas at STP

I've worked all of these questions and I'm trying to see if I'm right, and if not, where I went wrong.

It would be nice if you would show your work. Otherwise, we must work all of them too and it takes up so much of our time typing that it takes away from other students. 1.08 grams CO2? We won't have the slightest idea where you went wrong if we don't see your work.

To determine the number of grams of CO2 in 550 mL of gas at STP (Standard Temperature and Pressure), we can use the concept of molar mass and the ideal gas law. Here are the steps to find the answer:

1. Convert the volume from milliliters (mL) to liters (L):
Since 1 L = 1000 mL, divide 550 mL by 1000 to get the volume in liters.
550 mL ÷ 1000 = 0.55 L

2. Calculate the number of moles of CO2 using the ideal gas law:
The ideal gas law equation is PV = nRT, where:
P = pressure in atmospheres (atm)
V = volume in liters (L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (K)

At STP, the pressure is 1 atm and the temperature is 273 K.
Plug in the known values:
1 atm × 0.55 L = n × 0.0821 L·atm/(mol·K) × 273 K

Solve for n:
n = (1 atm × 0.55 L) / (0.0821 L·atm/(mol·K) × 273 K)
n ≈ 0.022 mol

3. Determine the molar mass of CO2:
CO2 has a molar mass of 44 g/mol. This means that one mole of CO2 weighs 44 grams.

4. Calculate the mass of CO2:
Multiply the number of moles (0.022 mol) by the molar mass (44 g/mol):
Mass = 0.022 mol × 44 g/mol
Mass ≈ 0.968 g

Therefore, there are approximately 0.968 grams of CO2 in 550 mL of gas at STP.

If you have already worked through these steps and arrived at a different answer, please double-check your calculations to spot any potential errors.