6
7
10
Mass of oxygen : 54 g
Conservation of mass applies to a closed system, where the masses before and after the reaction are the same
Reaction
mass before reaction = mass after reaction
mass C + mass O₂= mass CO₂
Answer:
Unsaturated solution.
Explanation:
At 60°C, 100.0g of water can dissolve 110g of KNO₃.
By definition, if you add 110g of KNO₃, the solution will be saturated, if you add more than 110g, the solution becomes supersaturated (That means crystals of solute will form), if you add less than 110g, the solution is unsaturated.
In the problem, you are adding 80g of KNO₃(s), that means you made a unsaturated solution.
2) One mole of gas occupies a volume of one liter.
3) Pressure is 1.0 atmosphere.
4) Volume is 2.4 liters
The reaction is at equilibrium at 1,000 K. The equilibrium constant of the reaction is 3.90. At equilibrium, the concentrations are as
follows.
[CO] = 0.30 M
[H2] = 0.10 M
[H20] = 0.020 M
What is the equilibrium concentration of CH, expressed in scientific notation?
0.0059
5.9 x 10-2
0.059
5.9 x 102
Answer: The equilibrium concentration of , expressed in scientific notation is
Explanation:
Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.
The given balanced equilibrium reaction is,
At eqm. conc. (0.30) M (0.10) M (x) M (0.020) M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
By solving the term 'x', we get :
x = 0.059 M=
Thus, the concentrations of at equilibrium is :
Concentration of = (x) M =
The equilibrium concentration of , expressed in scientific notation is
Answer:B
Explanation:B
B. kidneys
C. stomach
D. small intestine