Determine the pressure CHANGE when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C.

Answer 1

To determine the pressure change when a constant volume of gas is heated, we can use the ideal gas law:

PV = nRT

Where:
P = pressure
V = volume (constant in this case)
n = number of moles of gas (constant in this case)
R = ideal gas constant
T = temperature in Kelvin

First, we need to convert the initial and final temperatures to Kelvin:
Initial temperature = 20.0 °C = 20.0 + 273.15 = 293.15 K
Final temperature = 30.0 °C = 30.0 + 273.15 = 303.15 K

We can then set up an equation to represent the initial and final states of the gas using the ideal gas law:

P1V = nRT1
P2V = nRT2

Since V, n, and R are constant, we can simplify the equation to:

P1/T1 = P2/T2

Substitute in the values for initial and final pressure and temperature:

1.00 atm / 293.15 K = P2 / 303.15 K

Now, solve for P2:

P2 = (1.00 atm) * (303.15 K) / 293.15 K
P2 = 1.03 atm

The pressure change when the gas is heated from 20.0 °C to 30.0 °C is 0.03 atm (1.03 atm - 1.00 atm).