A commercial refrigerator unit accidentally releases 12.5 L of ammonia gas at SATP. Determine the mass and number of molecules of ammonia gas released.
Please if possible show the steps because I have an exam in an hour and I was trying this question and Im clueless.
Please help!
Thanks alot!
Better check your formulas
1 mole of gas at STP occupies 22.4L
So, you have
12.5/22.4 * 6.023*10^23 molecules
and convert moles to grams for mass
thanks but i received this after the exam
dfgr
To determine the mass and number of molecules of ammonia gas released, we need to use the ideal gas law equation, which relates the pressure, volume, temperature, and number of molecules of a gas.
The ideal gas law equation is expressed as follows:
PV = nRT
Where:
- P is the pressure of the gas (in pascals)
- V is the volume of the gas (in cubic meters)
- n is the number of moles of gas
- R is the ideal gas constant (8.314 J/mol·K)
- T is the temperature of the gas (in Kelvin)
In this case, the ammonia gas is released at SATP (Standard Ambient Temperature and Pressure). SATP conditions are defined as a temperature of 25°C (298.15 K) and a pressure of 1 atmosphere (101.325 kPa).
Given that the volume of ammonia gas released is 12.5 L, we need to convert it to cubic meters by dividing it by 1000:
V = 12.5 L / 1000 = 0.0125 m^3
Next, we substitute the known values into the ideal gas law equation:
PV = nRT
(101.325 kPa) * (0.0125 m^3) = n * (8.314 J/mol·K) * (298.15 K)
Simplifying the equation:
n = (101.325 kPa * 0.0125 m^3) / (8.314 J/mol·K * 298.15 K)
Now, we can solve for the number of moles (n):
n = (1.2665625 kPa*m^3) / (8.314 J/mol·K * 298.15 K)
n ≈ 0.0005096 moles
To find the mass, we can use the molar mass of ammonia (NH3), which is 17.031 g/mol. Multiplying the number of moles by the molar mass gives us the mass of ammonia:
Mass = n * Molar mass
Mass = 0.0005096 moles * 17.031 g/mol
Mass ≈ 0.008677 g
Finally, to determine the number of molecules, we can use Avogadro's number (6.022 × 10^23 molecules/mol):
Number of molecules = n * Avogadro's number
Number of molecules ≈ 0.0005096 moles * (6.022 × 10^23 molecules/mol)
Number of molecules ≈ 3.070 × 10^20 molecules
So, approximately 0.008677 grams of ammonia gas and about 3.070 × 10^20 molecules of ammonia gas were released.