One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 6.43 liters against a constant external pressure of 1.00 atm. how much work (in joules) is performed on the surroundings? ignore significant figures for this problem. (t = 300 k; 1 l·atm = 101.3 j)

-550.059 J

Explanation:

To calculate the amount of work done for an isothermal process is given by the equation:

W = amount of work done = ?

P = pressure = 1.00 atm

= initial volume = 1.00 L

= final volume = 6.43 L

Putting values in above equation, we get:

To convert this into joules, we use the conversion factor:

So,

The negative sign indicates the system is doing work.

Hence, the work done on the surroundings is -550.059 J

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

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