Question

Calculate the pressure (in atm) exerted by 4.2 g of carbon dioxide (CO₂) in a container with a 2 L volume at 18 °C.

a) 0.5 atm
b) 1.0 atm
c) 1.5 atm
d) 2.0 atm

Answer 1

To find the pressure exerted by the CO₂, convert the mass to moles, the temperature to Kelvin, then use the ideal gas law to solve for pressure. The results with given units and values indicate a pressure of about 1.2 atm, but this answer isn't listed in the options, suggesting a potential need for reevaluation or considering answer rounding.

Step-by-step explanation:

To calculate the pressure exerted by 4.2 g of CO₂ at 18 °C in a 2 L container, we can use the ideal gas law PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, convert the mass of CO₂ to moles:
n = mass / molar mass = 4.2 g / 44.01 g/mol = 0.095 moles of CO₂.

Next, convert the temperature to Kelvin:
T = 18 °C + 273.15 = 291.15 K.

Now, using R = 0.0821 L·atm/mol·K for the gas constant, solve for P:
P = nRT / V = (0.095 moles × 0.0821 L·atm/mol·K × 291.15 K) / 2 L = 1.2 atm.

However, 1.2 atm is not one of the given options. Therefore, calculations should be reviewed or an approximation could be considered if answers are rounded.