An 80.0-gram sample of a gas was heated from 25 °c to 225 °c. during this process, 346 j of work was done by the system and its internal energy increased by 7845 j. what is the specific heat of the gas?

The specific heat of the gas: c = 0.5119 J / g °C

The laws of thermodynamics 1 state that: energy can be changed but cannot be destroyed or created

The equation is:

Energy owned by the system is expressed as internal energy (U)

This internal energy can change if it absorbs heat Q (U> 0), or releases heat (U <0). Or theinternal energy can change if the system does work or accepts work (W)

The sign rules for heat and work are set as follows:

Heat can be calculated using the formula:

Q = heat, J

m = mass, g

c = specific heat, joules / g ° C

∆T = temperature difference, ° C / K

An 80.0-gram sample of a gas was heated from 25 ° C to 225 ° C

then the heat received:

Q = m. c ΔT

Q = 80. c. (225-25)

Q = 80. c. 200

Q = 16000c J

346 J of work was done by the system, then

W = - 346 J

its internal energy is increased by 7845 J, then

ΔU = 7845 J

So the thermodynamic equation:

ΔU = Q - W

7845 = 16000c - 346

8191 = 16000c

c = 0.5119 J / g °C

the difference between temperature and heat

Specific heat

relationships among temperature, heat, and thermal energy.

When heat is added to a substance