A group of students are studying how different stimuli affect the growth of plants. They place a growth lamp next to a plant tha
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The given question is incomplete. The complete question is :
Carbon tetrachloride can be produced by the following reaction:
Suppose 1.20 mol of and 3.60 mol of
were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.72 mol of
. Calculate equilibrium constant at the unknown temperature.
Answer: The equilibrium constant at unknown temperature is 0.36
Explanation:
Moles of = 1.20 mole
Moles of = 3.60 mole
Volume of solution = 1.00 L
Initial concentration of =
Initial concentration of =
The given balanced equilibrium reaction is,
Initial conc. 1.20 M 3.60 M 0 0
At eqm. conc. (1.20-x) M (3.60-3x) M (x) M (x) M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
Given :Equilibrium concentration of , x =
Thus equilibrium constant at unknown temperature is 0.36
First, find the number of moles for each element. The molar mass for nitrogen is 14 g/mol and that of hydrogen is 1 g/mol.
1.40 g N / 14 g/mol = 0.1 mol N
0.20 g H / 1 g/mol = 0.2 mol H
Find the mole ratio. Divide both numbers with the much lower value. In this case, it is 0.1 mol N.
For N: 0.1 ÷ 0.1 = 1
For H: 0.2÷0.1 = 2
Thus, the empirical formula is .