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
Write the balanced equation.
Before the reaction, determine the pressure from the sum of the partial pressures
partial pressure= nRT/V of each gas, then sum them.
You will have to then see what happens to the gasses: Did the ratio of the volumes change in the reaction. And, was all the reactants used up?
To write the balanced equation for the reaction, we need to determine the products formed when NO reacts with O2. The balanced equation will show the mole ratio between reactants and products.
Given:
NO(g) + O2(g) -> ???
To balance this equation, we can start by counting the number of each type of atom on each side of the equation.
For NO:
- Nitrogen (N): 1
- Oxygen (O): 1
For O2:
- Oxygen (O): 2
Now, compare the number of atoms on each side and adjust coefficients as needed to make them equal.
The balanced equation for the reaction is:
2NO(g) + O2(g) -> 2NO2(g)
Now, let's move on to calculate the total pressure in the cylinder at 298 K after the reaction is complete.
To do this, we need to determine the partial pressure of each gas before the reaction, then calculate the total pressure after the reaction.
Before the reaction, we only have NO(g) present in the cylinder with a quantity of 0.176 mol. The volume of the cylinder is given as 5.00 L.
To find the partial pressure of NO, we can use the ideal gas law equation:
PV = nRT
Rearranging the equation to solve for pressure (P), we have:
P = (nRT) / V
Plugging in the values:
P(NO) = (0.176 mol * 0.0821 atm/mol·K * 298 K) / 5.00 L
Calculate P(NO) = 1.632 atm
Now, after the reaction is complete, the NO and O2 have reacted to form NO2. The total moles of gas in the cylinder remain constant at 0.176 mol.
Since the volume is constant and the temperature is constant, we can assume the total pressure is the sum of the partial pressures of NO2 and any remaining NO gas.
P(total) = P(NO2) + P(NO)
To calculate P(NO2), we need to know the mole ratio between NO and NO2. From the balanced equation, we can see that 2 mol of NO produces 2 mol of NO2.
Therefore, the mole ratio of NO2 to NO is 1:1.
Since the total quantity of gas (0.176 mol) remains the same, we have 0.176 mol of NO2.
Using the ideal gas law again, we can calculate P(NO2) as follows:
P(NO2) = (0.176 mol * 0.0821 atm/mol·K * 298 K) / 5.00 L
Calculate P(NO2) = 1.632 atm
The partial pressure of NO remains the same, as it did not react or change in quantity.
Therefore, P(NO) = 1.632 atm
Now, we can calculate the total pressure:
P(total) = P(NO2) + P(NO) = 1.632 atm + 1.632 atm
Calculate P(total) = 3.264 atm
So, the total pressure in the cylinder at 298 K after the reaction is complete is 3.264 atm.