A different rigid 5.00L cylinder contains 0.176mol of NO(g) at 298 k. A 0.176mol sample of 02(g) is added to the cylinder, where a reaction occurs to produce NO2(g)
(d) write the balanced equation for the reaction.
(e) calculate the total pressure, in atm, in the cylinder at 298k after the reation is complete
1.29 atm
(d) The balanced equation for the reaction is:
2 NO(g) + O2(g) -> 2 NO2(g)
(e) To calculate the total pressure in the cylinder after the reaction is complete, we need to make use of the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, we need to calculate the initial pressure of the NO(g) in the cylinder. Since the volume and number of moles are given, we can use the ideal gas law equation to find the initial pressure:
P1V1 = n1RT
P1 = n1RT / V1
= (0.176 mol)(0.0821 L.atm/mol.K)(298 K) / 5.00 L
P1 = 0.0173 atm
The initial pressure of the NO(g) in the cylinder is 0.0173 atm.
Next, we need to consider the reaction that occurs. The 0.176 mol of O2(g) reacts with 0.176 mol of NO(g) to produce 0.352 mol of NO2(g).
Since volume and moles are constant in this case, the total pressure in the cylinder after the reaction would remain the same as the initial pressure.
Therefore, the total pressure in the cylinder at 298K after the reaction is complete is also 0.0173 atm.
To write the balanced equation for the reaction, let's break down the information given:
Initial gases:
NO(g) - 0.176 mol
O2(g) - 0.176 mol
From the information, we know that the reaction occurs to produce NO2(g). To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation.
The balanced equation for the reaction is:
2NO(g) + O2(g) -> 2NO2(g)
Now, to calculate the total pressure in the cylinder at 298 K after the reaction is complete, we need to consider the ideal gas law:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature
We have the volume of the cylinder (5.00 L), the number of moles of each gas (0.176 mol), and the temperature (298 K). We can assume the pressure after the reaction is complete is the same for all gases present. Therefore, we can calculate the total pressure by summing the partial pressures of each gas.
First, let's find the partial pressure of NO(g):
P(NO) = (n(NO) * R * T) / V
P(NO) = (0.176 mol * 0.0821 L·atm/mol·K * 298 K) / 5.00 L
Next, let's find the partial pressure of O2(g):
P(O2) = (n(O2) * R * T) / V
P(O2) = (0.176 mol * 0.0821 L·atm/mol·K * 298 K) / 5.00 L
Finally, let's find the total pressure by summing the partial pressures:
Total Pressure = P(NO) + P(O2)
By substituting the values we calculated for P(NO) and P(O2) into the equation, we can find the total pressure in the cylinder at 298 K after the reaction is complete.