An ideal gas is enclosed in a cylinder with a movable piston on top of it. The piston has a mass of 8,000 g and an area of 5.00 cm2 and is free to slide up and down, keeping the pressure of the gas constant.

(a) How much work is done on the gas as the temperature of 0.230 mol of the gas is raised from 25.0°C to 290°C?
J

(b) What does the sign of your answer to part (a) indicate?
The surroundings do positive work on the gas. There is no work done, by the gas or the surroundings. The gas does positive work on its surroundings

1,000

To calculate the work done on the gas, we can use the equation:

Work = Pressure * Change in Volume

First, let's determine the change in volume. Since the pressure of the gas is constant, we can use the ideal gas law to find the initial volume and final volume of the gas.

The ideal gas law is given as:

PV = nRT

Where:
P = Pressure (constant)
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature

Rearranging the equation, we can write:

V = nRT / P

Using the given values:

Moles of gas (n) = 0.230 mol
Initial temperature (T1) = 25.0°C = 25.0 + 273.15 = 298.15 K
Final temperature (T2) = 290°C = 290 + 273.15 = 563.15 K
Pressure (P) = constant

Calculating the initial volume (V1):

V1 = (0.230 mol * 0.0821 L·atm/mol·K * 298.15 K) / P

Similarly, calculating the final volume (V2):

V2 = (0.230 mol * 0.0821 L·atm/mol·K * 563.15 K) / P

Now, we need to find the change in volume:

Change in Volume = V2 - V1

Next, we can calculate the work done on the gas using the formula:

Work = Pressure * Change in Volume

Lastly, we need to convert the units to J (Joules).

Now that we have the general steps to solve the problem, you can go ahead and plug in the values to calculate the work done on the gas in Joules (J).