5. What is the pressure of a 5.0 L container which contains 3.0 moles of a gas at a temperature of 0°C? Note: Use Ideal gas law. R=8.31 (kPax L/mol x K)

P = 1361.17 KPa

Explanation:

Given data:

Mass of sample = 3.0 mol

Pressure of sample = ?

Volume of gas = 5.0 L

Temperature of gas = 0°C

Solution:

Pressure of gas:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 8.31 KPa.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

0+273 = 273 K

by putting values,

P × 5.0 L = 3.0 mol × 8.31 KPa.L/ mol.K  × 273 K

P = 6805.89 KPa.L/ 5.0 L

P = 1361.17 KPa

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)

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