A sample of 88.0 g CO2 is held at 291 K in a 40.0 L container. What is the pressure this gas exerts on the container. Express yo
1 answer:
Result:- 121 kPa.
Solution:- The parameters mass, temperature, and volume for carbon dioxide gas are given, and we are tasked with determining the pressure exerted by this gas on the container.
This is based on the ideal gas law equation, PV = nRT.
Where P stands for pressure in atm, V is the volume in liters, n is the gas moles, R is the universal gas constant with its value and T is the temperature in Kelvin.
Data provided:- mass = 88.0 g
T = 291 K
V = 40.0 L
P =?
We must convert mass into moles by dividing the mass by molar mass, where the molar mass of carbon dioxide is 44.01 grams per mole.
n = 2.00 mol
Reorganizing the equation for pressure gives us:
Let’s substitute the values and calculate for P.
P = 1.1946 atm
Since the question requests the answer in kPa, we need to convert atm to kPa.
1 atm = 101.325 kPa
Thus,
= 121 kPa
Consequently, the pressure this gas applies on the container is 121 kPa.
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Response: The moles in 369 grams of calcium hydroxide are 4.98 moles
Reasoning: Given,
Mass of calcium hydroxide = 369 g
Molar mass of calcium hydroxide = 74.093 g/mole
Formula used:
Now substituting the provided values into this formula, you will find the moles of calcium hydroxide.
Thus, the number of moles in 369 grams of calcium hydroxide is, 4.98 moles