(CH3)N2H2(l) + 2N204(g) = 3N2(g) + 4H2O(l) + 2CO2(g).
consider the reaction b2n 150g of liquid (CH3)N2H2 & 80L of N2O4 at 27 degree celcius & a pressure of 2 atm. The gases produced are collected at 27 degree celsius in an evacuated 250L. Calculate:
a) Partial pressure of nitrogen produced.
You need to do the following:
1. Convert 80L N2O4 at the conditions listed to moles. Use PV = nRT and solve for n.
2. Use stoichiometry to determine the moles N2 produced. Here is an example problem, worked, that shows how to do stoichiometry.
http://www.jiskha.com/science/chemistry/stoichiometry.html
3. Use PV = nRT to convert moles N2O4 at whatever conditions you wish (which the problem doesn't make clear) and solve for P.
By the way, note the correct spelling of celsius.
To calculate the partial pressure of nitrogen produced, we need to use the ideal gas law. The ideal gas law states that the product of pressure (P) and volume (V) is equal to the number of moles of gas (n) multiplied by the gas constant (R) and temperature (T). The equation is as follows:
PV = nRT
First, let's calculate the number of moles of nitrogen produced using the given information. From the balanced equation, we can see that 3 moles of nitrogen gas (N2) are produced for every mole of (CH3)N2H2(l) reacted.
Given that we have 150g of (CH3)N2H2, we need to convert this to moles. The molar mass of (CH3)N2H2 is:
(1 x 12.01) + (6 x 1.01) + (2 x 14.01) = 62.09 g/mol
Using the molar mass, we can calculate the moles of (CH3)N2H2:
moles of (CH3)N2H2 = mass / molar mass = 150g / 62.09 g/mol
Now, let's find the moles of nitrogen gas:
moles of N2 = moles of (CH3)N2H2 x (3 moles N2 / 1 mole (CH3)N2H2)
Next, we need to calculate the moles of nitrogen gas produced from the N2O4 reactant. From the balanced equation, we can see that 2 moles of nitrogen gas (N2) are produced for every mole of N2O4 reacted.
Given that we have 80L of N2O4, we need to convert this to moles using the ideal gas law. Rearranging the ideal gas law equation, we have:
n = PV / RT
where P is the pressure, V is the volume, R is the gas constant, and T is the temperature (in Kelvin).
But before we proceed with the calculation, we need to convert the temperature to Kelvin. The equation is:
T(K) = T(°C) + 273.15
So, T = 27 °C + 273.15 = 300.15 K
Now let's calculate the moles of N2O4:
n(N2O4) = PV / RT = (2 atm) * (80L) / [(0.0821 L.atm/mol.K) * (300.15 K)]
Finally, let's calculate the total moles of nitrogen gas produced:
total moles of N2 = moles of N2 + moles of N2O4
Now that we have the total moles of nitrogen gas, we can calculate the partial pressure of nitrogen using the ideal gas law. We can assume that the total volume of the gases is equal to the volume of the evacuated container, which is given as 250L.
P(N2) = (moles of N2 * R * T) / V
Let's substitute the values into the equation and calculate the partial pressure of nitrogen gas.