Answer:
K = 137.55 atm/M.
Explanation:
- The relationship between gas pressure and the concentration of dissolved gas is given by Henry’s law:
<em>P = (K)(C)</em>
where P is the partial pressure of the gaseous solute above the solution (P = 1.0 atm).
k is a constant (Henry’s constant).
C is the concentration of the dissolved gas (C = 7.27 x 10⁻³ M).
∴ K = P/C = (1.0 atm)/(7.27 x 10⁻³ M) = 137.55 atm/M.
Answer:
7,94 minutes
Explanation:
If the descomposition of HBr(gr) into elemental species have a rate constant, then this reaction belongs to a zero-order reaction kinetics, where the r<em>eaction rate does not depend on the concentration of the reactants. </em>
For the zero-order reactions, concentration-time equation can be written as follows:
[A] = - Kt + [Ao]
where:
- [A]: concentration of the reactant A at the <em>t </em>time,
- [A]o: initial concentration of the reactant A,
- K: rate constant,
- t: elapsed time of the reaction
<u>To solve the problem, we just replace our data in the concentration-time equation, and we clear the value of t.</u>
Data:
K = 4.2 ×10−3atm/s,
[A]o=[HBr]o= 2 atm,
[A]=[HBr]=0 atm (all HBr(g) is gone)
<em>We clear the incognita :</em>
[A] = - Kt + [Ao]............. Kt = [Ao] - [A]
t = ([Ao] - [A])/K
<em>We replace the numerical values:</em>
t = (2 atm - 0 atm)/4.2 ×10−3atm/s = 476,19 s = 7,94 minutes
So, we need 7,94 minutes to achieve complete conversion into elements ([HBr]=0).
Answer:
The alkaline hydrolysis of ester is known as saponification. When ester is heated with aqueous NaOH, sodium salt of acid and alcohol are formed.
I believe the end result is still 83 moles since there is never an amount of sulfur atoms added to the initial amount, but rather oxygen and water is repeatedly added to it. To find it's weight, first find the molar mass of H2SO4:
H2 + S + O4 = 2.00 + 32.1 + 64.0 = 98.1 g/mol
and mass = (98.1 g/mol)(83 mol) = 8142.3 g
rounded to 8.1 x 10^3 g assuming 100% yield?
Answer:
a. 1.00 x 10⁴ J = 10.0 kJ
b. 1.42 x 10⁴ J = 14.2 kJ
Explanation:
Given the change in temperature during the reaction and assuming the volume of water and density remains constant, the change in enthalpy for the reaction will be given by
ΔHxn = Q = mCΔT where,
m= mass of water
C= specific heat of water, and
ΔT= change in temperature
a. mH₂O = 400.0 mL x 1.00g/mL = 400.00 g
Q = ΔHrxn = 400.00g x 4.184 J/gºC x 6.00 ºC = 1.00 x 10⁴ J = 10.0 kJ
b. mH₂O = 200.0 mL x 1.00 g/mL = 200.0 g
Q = ΔHrxn = 200.00 g x 4.184 J/gºC x 17.0ºC = 1.42 x 10⁴ J = 14.2 kJ
