A substance (CD) decomposes into C and D.
CD(g) C(g) + D(g)
At the temperature of the experiment, 15.0 percent of CD is decomposed when equilibrium is established.
a) If the initial concentration of CD is 0.200 mol/L, what are the equilibrium concentrations of CD, C and D?
I wanted to know the steps of how to calculate this...
if 15 percent is cecomposed, then .85*.200M is the concentration of CD, and .15*.200 is the concentration of C, and D.
Check my thinking.
yes it is thank you very much
The equation is
2NH3 <=> N2 + 3H2
1 mole of NH3 injected intoa 1L flask
0.3 moles of H2 was found
the concentration of N2 at equlibrium is 0.1M
how do I find the concentration of NH3 at equlibrium?
answered above.
To find the concentration of NH3 at equilibrium, we need to use the stoichiometry of the reaction and the information given.
The balanced equation is:
2NH3 ⇌ N2 + 3H2
We are given that 1 mole of NH3 is injected into a 1L flask and the concentration of N2 at equilibrium is 0.1M.
Let's assume x mol/L of NH3 has reacted.
At equilibrium, the concentration of N2 is 0.1M, which means it has been formed from the reaction. According to the stoichiometry of the reaction, the formation of 1 mole of N2 corresponds to the consumption of 2 moles of NH3.
Since 2 moles of NH3 react to form 1 mole of N2, the concentration of NH3 at equilibrium will be x - 2x, as the reaction has consumed 2x moles of NH3 to form x moles of N2.
Given that the concentration of N2 at equilibrium is 0.1M, we can set up an equation:
0.1M = x - 2x
Simplifying the equation, we get:
0.1M = -x
Rearranging the equation, we find:
x = -0.1M
Since we cannot have a negative concentration, it means that no NH3 is present at equilibrium. Therefore, the concentration of NH3 at equilibrium is 0M.
Note: In this particular case, it is important to consider the extent of the reaction. If the extent of the reaction is small, the assumption that x is small compared to the initial concentration of NH3 is valid. However, if the reaction proceeds to a larger extent and the equilibrium concentration of NH3 is significant, this assumption may not be valid and a more precise calculation method is required.