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A 3.4 g sample of carbon dioxide (#CO_2#) gas is confined to a 450 mL rigid container at 55 deg C. How can you determine the pressure in the container?

Answer 1

Wyatt Adkins

Use the Ideal Gas Law, #P=(nRT)/V#

#P=(3.4*g)/(44.0*g*mol^-1)xx(0.0821*L*atm)/(K*mol)xx328*Kxx1/(0.45*L)#

#~=# #5*atm#

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Answer 2

Naomi Aronson

You can determine the pressure in the container using the ideal gas law equation: PV = nRT. First, calculate the number of moles of CO2 using the formula n = m/M, where m is the mass of CO2 (3.4 g) and M is the molar mass of CO2 (44.01 g/mol). Then, rearrange the ideal gas law equation to solve for pressure (P = nRT/V), where P is pressure, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), T is the temperature in Kelvin (55°C + 273.15), and V is the volume in liters (450 mL converted to L). Substituting the known values will give you the pressure in the container.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.