To calculate the new pressure, we need to use the ideal gas law, which states:
PV = nRT
Where: P = Pressure V = Volume n = Number of moles of gas R = Ideal gas constant (0.0821 L·atm/(mol·K)) T = Temperature (in Kelvin)
First, let's convert the initial volume to liters: V1 = 50 cubic centimeters = 50 mL = 0.05 L
The initial pressure is given as "mmHg," which stands for millimeters of mercury. We need to convert it to atmospheres (atm) for consistency. The conversion factor is: 1 atm = 760 mmHg
Next, let's convert the temperature to Kelvin: 0 °C = 273.15 K
Using the ideal gas law, we can solve for the initial pressure (P1): P1 * V1 = n * R * T
Now, let's calculate P1: P1 = (n * R * T) / V1
Since we don't have the number of moles (n), we can't determine the exact pressure. We need additional information, such as the gas used or its molar mass.
Moving on to the second part of the question, we are given the new volume (V2 = 250 cubic centimeters = 0.25 L) while keeping the temperature constant at 0 °C (273.15 K). We can use the same equation and rearrange it to solve for the new pressure (P2):
P2 = (n * R * T) / V2
However, without knowing the number of moles or any other information, we cannot calculate the new pressure accurately.