Question

calculate pressure exerted by 1.255 mol of CI2 in a volume of 5.005 L at a temperature 273.5 k using ideal gas equation

Answer 1

The pressure is 5.62 atm.

Step-by-step explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

• P= ?
• V= 5.005 L
• n= 1.255 mol
• R= 0.082
  `(atm*L)/(mol*K)`
• T= 273.5 K

Replacing:

P* 5.005 L= 1.255 mol* 0.082
`(atm*L)/(mol*K)` *273.5 K

Solving:

`P=(1.255 mol* 0.082 (atm*L)/(mol*K) *273.5 K)/(5.005 L)`

P= 5.62 atm

The pressure is 5.62 atm.