consider the following chemical reaction:
2 H20 ---> 2H2 + O2
How many moles of H20 are required to form 1.8 L of O2 at a temperature of 315 K and a pressure of 0.957 atm?
I got 0.066 moles.
Correct?
Nope.
Do you have some reasoning that you followed you want to have critiqued?
To determine the correct answer, let's go through the steps together:
The given chemical reaction is:
2 H2O → 2 H2 + O2
We want to find out how many moles of H2O are required to produce 1.8 L of O2 at a temperature of 315 K and a pressure of 0.957 atm.
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in K)
In this case, we have:
P = 0.957 atm
V = 1.8 L
T = 315 K
R = 0.0821 L·atm/(mol·K)
Now, rearranging the ideal gas law equation to solve for n:
n = PV / RT
Substituting the given values:
n = (0.957 atm) * (1.8 L) / (0.0821 L·atm/(mol·K) * 315 K)
After performing the calculation, the result is approximately 0.087 moles (rounded to three decimal places).
Therefore, the correct answer is 0.087 moles of H2O are required to form 1.8 L of O2 at the given conditions.
So, the answer you provided, 0.066 moles, is not correct.