Use the equation to determine what volume of nitrous oxide can be produced from the decomposition of o.55 moles of ammonium nitrate useing the equation:
NH4NO3 (s)--> N2O (g) + 2H2O (g)
To determine the volume of nitrous oxide (N2O) produced from the decomposition of 0.55 moles of ammonium nitrate (NH4NO3), we need to use the balanced chemical equation:
NH4NO3 (s) → N2O (g) + 2H2O (g)
Step 1: Convert moles of ammonium nitrate (NH4NO3) to moles of nitrous oxide (N2O).
According to the balanced equation, 1 mole of NH4NO3 produces 1 mole of N2O. Therefore, if we have 0.55 moles of NH4NO3, we will have 0.55 moles of N2O.
Step 2: Convert moles of nitrous oxide (N2O) to volume using the ideal gas law equation.
The ideal gas law equation is given as:
PV = nRT
Where:
P = pressure (in Pascals or atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K for most calculations)
Assuming that the pressure and temperature are constant, we can simplify the equation to:
V = (nRT) / P
Step 3: Gather the necessary information to substitute into the equation.
Given:
n (moles) = 0.55 moles
R (ideal gas constant) = 0.0821 L·atm/mol·K (at standard temperature and pressure)
P (pressure) = Assuming it is at standard pressure (1 atm).
Step 4: Plug the values into the equation and solve for volume (V).
V = (0.55 moles * 0.0821 L·atm/mol·K * T K) / 1 atm
Note: Temperature (T) needs to be provided to determine the volume accurately. If the temperature is not given, a specific value needs to be assumed to calculate the volume accurately.
Once you have substituted the values into the equation and have a specific temperature, you can calculate the volume of nitrous oxide (N2O) produced.
Remember to include the appropriate units for pressure, volume, and temperature in the calculation.
Use this link and look at your last post just above this to see a discussion.
http://www.jiskha.com/science/chemistry/stoichiometry.html