Chemical reaction that absorbs heat from its environment
Method A is Convection
Method B is Conduction
Explanation:
From the problem, we can infer that method A is convection and method B is conduction.
Conduction, convection and radiation are the three main methods of heat transfer.
- Conduction and convection requires material medium to propagate.
- Radiation occurs in the absence of a material medium.
- Conduction mostly occurs in solid. Here, heat is transferred from one hot end to the cold end of the solid. The vibration of the particles in the hot end causes the transfer of kinetic energy to the cold end until thermal equilibrium is reached.
- In convection, heat is primarily transferred in fluids as a result of density differences. Convection involves the motion of the materials of the medium. Hot air is light and it rises whereas cold air is dense and it sinks.
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Answer:
T° freezing solution → -11.3°C
T° boiling solution → 103.1 °C
Explanation:
Assuming 100 % dissociation, we must find the i, Van't Hoff factor which means "the ions that are dissolved in solution"
This salt dissociates as this:
SnCl₄ (aq) → 1Sn⁴⁺ (aq) + 4Cl⁻ (aq) (so i =5)
The formula for the colligative property of freezing point depression and boiling point elevation are:
ΔT = Kf . m . i
where ΔT = T° freezing pure solvent - T° freezing solution
ΔT = Kb . m . i
where ΔT = T° boiling solution - T° boiling pure solvent
Freezing point depression:
0° - T° freezing solution = 1.86°C/m . 1.22 m . 5
T° freezing solution = - (1.86°C/m . 1.22 m . 5) → -11.3°C
Boiling point elevation:
T° boiling solution - 100°C = 0.512 °C/m . 1.22 m . 5
T° boiling solution = (0.512 °C/m . 1.22 m . 5) + 100°C → 103.1 °C
Answer: 0.422 M⁻¹s⁻¹
Explanation: <u>Reaction</u> <u>Rate</u> is the speed of decomposition of the reactant(s) per unit of time.
A <u>Rate</u> <u>Law</u> relates concentration of reactants, rate reaction and rate constant:
![r=k[A]^{x}[B]^{y}](https://tex.z-dn.net/?f=r%3Dk%5BA%5D%5E%7Bx%7D%5BB%5D%5E%7By%7D)
where
[A] and [B] are reactants concentration
x and y are reaction order, not related to the stoichiometric coefficients
k is rate constant
r is rate
Before calculating rate constant, first we have to determine reaction order.
In this question, the reactio order is 2. So, the rate law for it is
![-\frac{d[A]}{dt} =k[A]^{2}](https://tex.z-dn.net/?f=-%5Cfrac%7Bd%5BA%5D%7D%7Bdt%7D%20%3Dk%5BA%5D%5E%7B2%7D)
and the integrated formula is
![\frac{1}{[A]} =\frac{1}{[A]_{0}} +kt](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7B%5BA%5D%7D%20%3D%5Cfrac%7B1%7D%7B%5BA%5D_%7B0%7D%7D%20%2Bkt)
in which
[A]₀ is initial concentration of reactant
Then, using initial concentration at initial time and final concentration at final time:
k = 0.422
The rate constant for the reaction is 0.422 M⁻¹.s⁻¹
Answer:
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