CaCO3 can be roasted to produce CaO ans CO2 this reaction is carried out in flask connected to an open end Mercury manometer the atmospheric presure in 762tor if the pressure of the CO2 produced is 0.254 determine the total pressure
To determine the total pressure, we need to consider the pressure of the CO2 produced (0.254 atm) and the atmospheric pressure (762 torr).
Note: We need to convert the pressure units before adding them together because they are in different units.
1 torr is equal to 1/760 atm. Therefore, 762 torr is equal to 762/760 = 1.003 atm.
Now we can add the pressures together:
Total Pressure = Pressure of CO2 + Atmospheric pressure
Total Pressure = 0.254 atm + 1.003 atm
Total Pressure = 1.257 atm
Therefore, the total pressure is 1.257 atm.
To determine the total pressure in the flask, we need to add the pressure of the CO2 produced to the atmospheric pressure.
Let's start by understanding the information given in the question:
- The atmospheric pressure is given as 762 torr (torr is a unit of pressure).
- The pressure of the CO2 produced is given as 0.254 torr.
To calculate the total pressure, we simply add the pressure of the CO2 produced to the atmospheric pressure. Mathematically, it can be written as:
Total pressure = Atmospheric pressure + Pressure of CO2
Total pressure = 762 torr + 0.254 torr
Total pressure = 762.254 torr
Therefore, the total pressure in the flask is 762.254 torr.
0.254 what? mm, atm, kPa?
and you want the total pressure where? in the flask? I don't know what you mean by total pressure.