Use Arrhenius equation:
k = A*exp(-Ea/RT)
We have:
1.35x10^2/s = A*exp(-85600/(8.314*298.15))
or: A = 1.342x10^17/s
It is a piece of cake to calculate:
k = 1.342x10^17*exp(-85600/(8.314*348.15))
= 1.92x10^4/s
Answer:
130 g of sucrose
Explanation:
Boiling point elevation formula → ΔT = Kb . m
ΔT = Boiling T° solution - Boiling T° pure solvent → 0.39°C
0.39°C = 0.513°C/m . M
m = 0.760 mol/kg → molality = moles of solute / 1kg of solvent
Let's determine the moles of solute → molality . kg
0.760 mol/kg. 0.5 kg = 0.380 moles
If we convert the moles to mass, we'll get the answer
0.380 mol . 342.30 g/mol = 130g
This is an incomplete question, here is a complete question.
The Henry's law constant for oxygen dissolved in water is 4.34 × 10⁹ g/L.Pa at 25⁰C.If the partial pressure of oxygen in air is 0.2 atm, under atmospheric conditions, calculate the molar concentration of oxygen in air-saturated and oxygen saturated water.
Answer : The molar concentration of oxygen is, 
Explanation :
As we know that,

where,
= molar solubility of
= ?
= partial pressure of
= 0.2 atm = 1.97×10⁻⁶ Pa
= Henry's law constant = 4.34 × 10⁹ g/L.Pa
Now put all the given values in the above formula, we get:


Now we have to molar concentration of oxygen.
Molar concentration of oxygen = 
Therefore, the molar concentration of oxygen is, 
Answer:
Number of protons = 52, Number of electrons = 52, Number of neutrons = 76
Explanation:
Hello!
To solve this problem we're going to use the
Charles' Law. This Law describes the relationship between
Volume and Temperature in an ideal gas. Applying this law we have the following equation:

So, the final temperature is
54,23 °CHave a nice day!