An 80.0 g sample of a gas was heated from 25 degree C to 225 degree C. During this process, 346 J of work was done by the system and its internal energy increased by 7495 J. What is the specific heat of the gas?
J/(g∗C)
you did not solve the whole problem!
To find the specific heat of the gas, we can use the equation:
ΔU = q + W
where ΔU is the change in internal energy of the gas, q is the heat absorbed by the gas, and W is the work done by the gas.
In this case, we are given:
ΔU = 7495 J (increase in internal energy)
W = 346 J (work done by the system)
To find q, we can rearrange the equation:
q = ΔU - W
q = 7495 J - 346 J
q = 7149 J
Next, we'll use the equation for specific heat:
q = mcΔT
where q is the heat absorbed, m is the mass of the gas, c is the specific heat of the gas, and ΔT is the change in temperature.
In this case, we are given:
q = 7149 J
m = 80.0 g
ΔT = (225 °C - 25 °C) = 200 °C
Rearranging the equation, we can solve for c:
c = q / (m * ΔT)
c = 7149 J / (80.0 g * 200 °C)
c = 0.447 J/(g∗C)
Therefore, the specific heat of the gas is 0.447 J/(g∗C).
To find the specific heat of the gas, we can use the formula:
q = m * C * ΔT
where:
q is the heat absorbed or released by the system,
m is the mass of the gas,
C is the specific heat of the gas, and
ΔT is the change in temperature.
In this case, we know the following values:
m = 80.0 g (mass of the gas)
ΔT = 225°C - 25°C = 200°C (change in temperature)
q = 7495 J (change in internal energy)
We want to find the specific heat, C. Rearranging the formula, we get:
C = q / (m * ΔT)
Substituting the given values:
C = 7495 J / (80.0 g * 200°C)
Now, let's calculate this:
C = 7495 J / (16000 J/°C)
C ≈ 0.47 J/(g∗°C)
Therefore, the specific heat of the gas is approximately 0.47 J/(g∗°C).
I believe this is
E2-E1 = delta E = q+w
dE = 7495
w is -346
q = 7495+346 = ?
Then q = mass gas x specific heat gas x (Tfinal-Tinitial)
Solve for specific heat gas.