Final answer:
The density of carbon dioxide gas at 285 K and 0.95 atm is 1.96 kg/m³.
Step-by-step explanation:
The density of a gas can be calculated using the ideal gas law equation, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. To calculate the density, we can rearrange the equation to solve for density (ρ), which is mass per unit volume. The equation becomes ρ = (PM) / RT, where PM is the molar mass of the gas. In this case, we are given the temperature and pressure of carbon dioxide gas. We can use the ideal gas law equation to calculate the density.
First, we need to convert the pressure from atm to Pa. 1 atm is approximately equal to 101325 Pa. So, the pressure of carbon dioxide gas is 0.95 atm * 101325 Pa/atm = 95858.75 Pa.
Next, we convert the temperature from Celsius to Kelvin. The temperature in Kelvin is equal to the temperature in Celsius plus 273.15. So, the temperature of carbon dioxide gas is 10°C + 273.15 = 283.15 K.
Now, we can substitute the values into the density equation. The molar mass of carbon dioxide gas is approximately 44.01 g/mol. Plugging in the values, we get ρ = (95858.75 Pa * 44.01 g/mol) / (8.314 J/(mol·K) * 283.15 K) = 1.956 kg/m³.