Hi,
I really need help with my lab report because Im completely stuck.
Its about the Ideal Gas behaviour.
I am given the mass of Nano2 (0.5044g) the temperature of n2 gas (21.2 C)
the temperature of water (21.9 C) the volume of n2 (186.1 ml) and the barometric pressure (753.06 torr).
I am asked to find the absolut temperature of the n2 gas, total gas pressure in the flask and degree of completion of reaction in percent.
Help is greatly appreciated!
Of course, I can help you with your lab report. To find the absolute temperature of the N2 gas, you need to convert the given temperature from Celsius to Kelvin. To do this, you can use the equation:
T(K) = T(C) + 273.15
So, to find the absolute temperature of the N2 gas, you will calculate:
T(N2 gas, K) = 21.2 + 273.15
Next, to calculate the total gas pressure in the flask, you need to consider the barometric pressure. The total gas pressure is the sum of the barometric pressure and the pressure due to the N2 gas. Since the pressure of N2 gas is given in torr, which is the same unit as barometric pressure, you can directly add the two pressures together. This can be expressed as:
Total pressure = Barometric pressure + Pressure of N2 gas
Substituting the given values:
Total pressure = 753.06 torr + (pressure of N2 gas)
Now, to find the pressure of the N2 gas, you can use the ideal gas law equation:
PV = nRT
Since you have the volume (V), mass (m), and temperature (T) of the N2 gas, you need to find the number of moles (n) before substituting it into the ideal gas law equation. To find the number of moles, you can use the formula:
n = (mass of N2 gas) / (molar mass of N2 gas)
The molar mass of N2 gas can be found in the periodic table, and it is about 28.01 g/mol.
Once you find the number of moles, you can substitute it into the ideal gas law equation along with the given volume and temperature to solve for the pressure of the N2 gas.
After calculating the pressure of the N2 gas, you can substitute it back into the previous equation to find the total gas pressure in the flask.
Finally, to find the degree of completion of reaction in percent, you need to know more information about the reaction and the stoichiometry involved. It would be helpful if you could provide more details about the reaction you are conducting so that I can assist you further in calculating the degree of completion.
I hope this explanation helps you in solving your lab report. Feel free to ask any further questions if needed.
Of course, I can help you with your lab report on the Ideal Gas behavior. Let's go step-by-step.
Step 1: Convert the given temperatures to Kelvin.
To convert Celsius to Kelvin, we add 273.15 to the given value.
Temperature of N2 gas = 21.2°C + 273.15 = 294.35 K
Temperature of water = 21.9°C + 273.15 = 295.05 K
Step 2: Convert the given volume of N2 gas to liters.
Volume of N2 gas = 186.1 ml = 186.1/1000 = 0.1861 L
Step 3: Calculate the absolute temperature of the N2 gas.
The absolute temperature is given by the formula: T = (P * V) / (n * R)
where T is the absolute temperature, P is the pressure, V is the volume, n is the number of moles, and R is the ideal gas constant.
To find the absolute temperature, we need to know the number of moles. Since we are not given the number of moles of N2, we can use the ideal gas equation PV = nRT to find it.
Step 4: Calculate the number of moles of N2.
PV = nRT
Rearranging the equation, n = (PV) / (RT)
Here, we know the pressure (753.06 torr), volume (0.1861 L), and temperature (294.35 K). The ideal gas constant R = 0.0821 L*atm/(mol*K).
n = (753.06 torr * 0.1861 L) / (0.0821 L*atm/(mol*K) * 294.35 K)
n = (139.8976666) / (24.207035)
n = 5.769 mol
Step 5: Calculate the absolute temperature of the N2 gas.
T = (P * V) / (n * R)
T = (753.06 torr * 0.1861 L) / (5.769 mol * 0.0821 L*atm/(mol*K))
T = (139.8976666) / (0.4748369)
T = 294.31 K (approx)
Therefore, the absolute temperature of the N2 gas is approximately 294.31 K.
Step 6: Calculate the total gas pressure in the flask.
The total gas pressure in the flask is the sum of the pressure contributed by N2 gas and the water vapor. The water vapor pressure can be determined using the vapor pressure table for water at 21.9°C (295.05 K).
According to the vapor pressure table, the vapor pressure of water at 21.9°C (295.05 K) is approximately 19.8 torr.
Total gas pressure = N2 gas pressure + water vapor pressure
Total gas pressure = 753.06 torr + 19.8 torr
Total gas pressure = 772.86 torr
Therefore, the total gas pressure in the flask is approximately 772.86 torr.
Step 7: Calculate the degree of completion of the reaction in percent.
Without further information about the reaction, it's not possible to determine the degree of completion. Please provide additional details about the reaction to proceed further.
I hope this step-by-step explanation helps you with your lab report. Let me know if you have any further questions.