Mass of gas is 300 gm and its specific heat at constant volume is 750 J/kg K. if gas is heated through 75°C at constant pressure of 105 N/{m^2}, it expands by volume
and the question is?
To find the change in volume of the gas, we need to use the ideal gas law equation, which states:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
However, since we are given the change in temperature at constant pressure, we can use a simplified version of the ideal gas law called Gay-Lussac's law of pressure-temperature relationship:
(P1/T1) = (P2/T2)
In this equation, P1 and T1 represent the initial pressure and temperature, and P2 and T2 represent the final pressure and temperature. We can rearrange this equation to solve for the final volume (V2) of the gas:
V2 = V1 * (T2/T1) * (P1/P2)
Given:
Mass (m) = 300 g = 0.3 kg
Specific heat at constant volume (Cv) = 750 J/kg K
Change in temperature (∆T) = 75°C
To find the final volume, we need to know the initial volume (V1) and the initial pressure (P1). Unfortunately, this information is not provided in the question. Can you please provide the values for the initial volume and pressure of the gas?