Acetic acid is a weak acid and sodium hydroxide is strong base. Salts of the two will hydrolyse to give basic solution. So, at neutral point, pH of the solution will be greater than 8.
air that is cooling will cause the highest pressure
Explanation:
This is because heat has to escape a certain area and if the heat can't escape then more and more pressure will build up in a area.
After alpha decay (234,90) remain from it
Answer:
-30.0 ºC
Explanation:
The freezing point depression of a solution is given by the relation:
ΔT = - Kf m, where Kf is the molal freezing point constant of water, and m is the molality of the solute.
The molality, in turn, is given by:
m = mol solute / Kg solvent
We are not given in this question the identity of the solute, but the most typical component in antifreeze is ethylene glycol, and that is what we are going to use here.
We now have all the information required to solve this question.
In 100 grams of fluid we have:
Molar mass ethylene glycol = 62.07 g/mol
mol ethyle glycol = 50 g / 62.07 g/mol = 0.81 mol
Kg solvent = 50 g/ 1000 g/ Kg = 0.050 Kg
m = 0.81 mol / 0.050 Kg = 16.1 m
ΔT = - Kf m = -1.86 ºC/m x 16.1 m = -30.0 ºC
Answer:
K= -0.286 Mol^-1.S^-1
Explanation:
FIRSTLY, WE WRITE A CHEMICAL REACTION EQUATION FOR THE REACTION BETWEEN OXALIC ACID AND POTASSIUM PERMANGANATE.
KMnO2(aq) + H2C2O4(aq) ----> Mn2+(aq) + CO2(g) + H2O(l)
(purple) (colorless)
THE RATE OF THE REACTION IS MEASURED AND MONITORED BY CHECKING FOR THE DISAPPEARANCE OF THE PURPLE COLOR OF THE POTASSIUM PERMANGANATE.
The rate of the reaction is given by : -Δ[KMnO4]/ΔT = -Δ[ H2C2O4]/ΔT = Δ[ Mn2+]/ΔT
When all of the purple color is gone, we can say that the reaction is finished and that the final concentration of the KMnO4 is now zero. Since the initial time for ΔT is zero, the equation for the rate of
disappearance of the potassium permanganate becomes:
Rate = Δ[KMnO4]/ΔT= (0-[initial KMnO4]) ÷ (elapsed time -0) = [Initial KMnO4 ] ÷ elapsed time
Hence, the rate of the chemical reaction is thus;
-1.3/5 = -0.26M/s
Now, to get the rate constant for the reaction, we need to know the rate law and this can be expressed as follows:
For a reaction A+B---> C The general rate law would be: Rate = k[A]^m[B]^n
In this particular case,
Rate =k [KMnO4][ H2C2O4]
Kindly note that m and n in this case is 1 each. We have calculated our rate from above. Hence:
-0.26 = k(1.3)(0.7)
k = -0.26÷(1.3)(0.7)
K= -0.286 Mol^-1.S^-1