a steel cylinder with nitrotgen hydrogen and ammonia gases is at 500C and 5.00 atm if patrtila pressure of nitrogen is 1850 mm Hg and hydrogen is 1150 mm Hg what is the partial pressure of ammonia in mm H</p>
Ptotal = PN2 + PH2 + PNH3
Substitute and solve for PNH3.
To find the partial pressure of ammonia, we need to use the ideal gas law. The ideal gas law equation is:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
Since we are given the temperature in degrees Celsius, we need to convert it to Kelvin by adding 273.15.
So let's start by converting the given temperature:
T = 500°C + 273.15 = 773.15 K
Now, according to Dalton's law of partial pressures, the sum of the partial pressures of all the gases in the cylinder will be equal to the total pressure.
Total pressure (P_total) = Partial pressure of nitrogen (P_nitrogen) + Partial pressure of hydrogen (P_hydrogen) + Partial pressure of ammonia (P_ammonia)
P_total = P_nitrogen + P_hydrogen + P_ammonia
We are given the total pressure:
P_total = 5.00 atm
Now, we need to convert the partial pressures of nitrogen and hydrogen to atm:
1 atm = 760 mm Hg
P_nitrogen = 1850 mm Hg * (1 atm / 760 mm Hg) = 2.4342 atm (rounded to four decimal places)
P_hydrogen = 1150 mm Hg * (1 atm / 760 mm Hg) = 1.5132 atm (rounded to four decimal places)
Now, we can substitute the known values into the equation and solve for the partial pressure of ammonia:
5.00 atm = 2.4342 atm + 1.5132 atm + P_ammonia
To find P_ammonia, we can rearrange the equation:
P_ammonia = 5.00 atm - (2.4342 atm + 1.5132 atm)
P_ammonia = 0.0526 atm (rounded to four decimal places)
Lastly, we convert the partial pressure of ammonia back to mm Hg:
P_ammonia = 0.0526 atm * (760 mm Hg / 1 atm) = 39.936 mm Hg (rounded to three decimal places)
Therefore, the partial pressure of ammonia is approximately 39.936 mm Hg.