the pressure of hydrogen gas in a constant volume cylinder is 4.25atm at 0 degrees celsius. what will the pressure be if the temp. is raised to 80 degress celsius? Also do we have to first convert celsius to kelvin?
See your last post above.
Yes, C must in kelvin.
To determine the pressure of hydrogen gas at a different temperature, you need to use the Ideal Gas Law, which states:
PV = nRT
Where:
P = Pressure
V = Volume (constant in this case)
n = Number of moles (constant in this case)
R = Ideal Gas Constant (constant)
T = Temperature in Kelvin
To convert Celsius to Kelvin, you need to add 273.15 to the Celsius value. So, in this case, we would add 273.15 to both the initial and final temperature.
Given that the pressure at 0 degrees Celsius is 4.25 atm, we can assume that these conditions are in equilibrium and we don't need to account for any changes in moles or volume.
Let's follow these steps to find the pressure at 80 degrees Celsius:
Step 1: Convert the initial and final temperatures to Kelvin.
Initial temperature (0 degrees Celsius + 273.15) = 273.15 K
Final temperature (80 degrees Celsius + 273.15) = 353.15 K
Step 2: Use the Ideal Gas Law equation to compare the two pressures.
(P1)(V) / (T1) = (P2)(V) / (T2)
Since V (volume) is constant, we can simplify the equation to:
P1 / T1 = P2 / T2
Step 3: Plug in the values into the equation:
(4.25 atm) / (273.15 K) = (P2) / (353.15 K)
Step 4: Solve for P2:
P2 = (4.25 atm) * (353.15 K) / (273.15 K)
By calculating this, you'll find that the pressure at 80 degrees Celsius will be approximately 5.49 atm.
So, yes, you must convert the temperature to Kelvin when using the Ideal Gas Law equation.
To calculate the pressure of hydrogen gas when the temperature is raised to 80 degrees Celsius, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the initial temperature from Celsius to Kelvin using the formula: K = °C + 273.15.
So, the initial temperature in Kelvin is:
T1 = 0°C + 273.15 = 273.15 K
Now, let's convert the final temperature from Celsius to Kelvin:
T2 = 80°C + 273.15 = 353.15 K
Since the cylinder is a constant volume cylinder, the volume (V) remains the same.
To find the relation between the initial pressure (P1) and final pressure (P2), we can rearrange the ideal gas law equation to solve for pressure:
P = nRT / V
Since the number of moles and volume remain constant, we can rewrite the equation as:
P1/T1 = P2/T2
Now, substitute the given values:
P1/273.15 K = P2/353.15 K
Solve for the final pressure (P2):
P2 = (P1 * 353.15 K) / 273.15 K
Let's calculate the final pressure using the given values:
P2 = (4.25 atm * 353.15 K) / 273.15 K
P2 ≈ 5.48 atm
Therefore, the pressure of hydrogen gas in the constant volume cylinder will be approximately 5.48 atm when the temperature is raised to 80 degrees Celsius.
Yes, we do need to convert the Celsius temperature to Kelvin before performing calculations using the ideal gas law equation. The ideal gas law equation requires temperature to be in Kelvin because the absolute temperature scale is used.