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.
You might be interested in
Answer :
The percentage ionic character (%IC) equals 10%, indicating the bond is mostly covalent with slight polarity.
Percent Ionic Character:
This reflects the fraction of ionic nature within a polar covalent bond. The formula for %IC (% ionic character) is:
Here, Xa is the electronegativity of atom A and Xb is that of atom B.
Given: The compound is TiAl₃.
Electronegativity of Ti = 2.0
Electronegativity of Al = 1.6 (as shown in the provided image)
Substitute these values into the formula:
The value of e⁻¹ equals 0.90.
Therefore, percent ionic character = (1 - 0.90) × 100
Percent Ionic Character = 10%
Because the % IC is only 10%, which is relatively low, the bond is classified as covalent with minimal polarity.
