Calculate the pressure exerted by 1.00 mol of CO2 in a 1.00 L vessel at 300 K, assuming that the gas behaves ideally.

24.6 atm

Explanation:

Step 1: Given and required data

Step 2: Calculate the pressure of carbon dioxide

Assuming ideal gas behavior, we will use the ideal gas equation.

P × V = n × R × T

P = n × R × T/V

P = 1.00 mol × 0.08206 atm.L/mol.K × 300 K/1.00 L

P = 24.6 atm

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)