dinitrogen pentoxide n2o5 decomposes by a first-order decomposition in chloroform solvent to yield NO2 and O2. The rate constant at 45°C is 6.2 x 10^-4 mins^-1. Calculate the volume of O2 obtained from the reaction of 1.00 mol N2O5 at 45°C and 770 mmHg after 20.0 hours.
N2O5 = 2 NO2 + 1/2 O2
Wouldn't this be
ln(No/N) = kt
You know No and k, t is given but change so k and t are in the same units. Solve for N = mols N2O5 at end of 20 hours, then take 1/2 that for mols O2 and use PV = nRT to calculate volume O2.
I keep getting 6.12 and the answer is suppose to be 6.8
To calculate the volume of O2 obtained from the reaction of 1.00 mol N2O5, we need to follow these steps:
Step 1: Calculate the number of moles of O2 produced.
From the balanced chemical equation, you can see that for every 1 mole of N2O5, we obtain 1/2 mole of O2. Therefore, if we have 1.00 mole of N2O5, we will produce 1/2 * 1.00 moles = 0.50 moles of O2.
Step 2: Use the ideal gas law to calculate the volume of O2.
The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
In this case, we are given the number of moles of O2 (0.50 moles), the temperature (45°C = 45 + 273 = 318 K), and the pressure (770 mmHg). We need to calculate the volume (V).
Step 3: Convert pressure to atm.
Since the ideal gas law uses pressure in atmospheres (atm), we need to convert the given pressure from mmHg to atm.
1 atm = 760 mmHg.
Therefore, 770 mmHg = 770/760 atm = 1.013 atm.
Step 4: Plug in the values into the ideal gas law equation and solve for V.
Using the ideal gas law equation PV = nRT, we can rearrange it to V = (nRT)/P.
V = (0.50 moles * 0.0821 L·atm/(K·mol) * 318 K) / 1.013 atm.
Now, calculate the volume by plugging in the values and solving the equation.