the dissociation of molecular iodine into iodine atoms is represented as: I2 =2I Suppose that .0256 mole of I2 was placed in a 2.30 L flask at 1000K. what is the intial concentration of the I2 before any reaction occurs?
M = moles/L; right?
To find the initial concentration of I2, we need to use the given information about the number of moles and the volume of the flask.
The equation for concentration (C) is:
C = n / V,
where C is the concentration, n is the number of moles, and V is the volume.
Given:
- Number of moles (n) = 0.0256 mole
- Volume (V) = 2.30 L
Substituting the values into the equation:
C = 0.0256 mole / 2.30 L
Using a calculator, we can find the initial concentration:
C = 0.01113 mole/L (rounded to five decimal places)
Therefore, the initial concentration of I2 before any reaction occurs is approximately 0.01113 mole/L.