How many molecules are in 3.5 moles of water? Fill in the chart to show your work. Then, solve the problem and answer the questi
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Answer: Concentrations of cyclohexane and methylcyclopentane at equilibrium are 0.0223 M and 0.0027 M respectively
Explanation:
Moles of cyclohexane = 0.069 mole
Volume of solution = 2.8 L
Initial concentration of cyclohexane =
The given balanced equilibrium reaction is,
cyclohexane ⇔ methylcyclopentane
Initial conc. 0.025 M 0
At eqm. conc. (0.025-x)M (x) M
The expression for equilibrium constant for this reaction will be,
K= methylcyclopentane / cyclohexane
Now put all the given values in this expression, we get :
By solving the term 'x', we get :
x = 0.0027
Concentration of cyclohexane at equilibrium = (0.025-x ) M = (0.025-0.0027) M = 0.0223 M
Concentration of methylcyclopentane at equilibrium = (x ) M = (0.0027) M
Answer:
The total photons required = 5.19 × 10²⁸ photons
Explanation:
Given that:
the radiation wavelength λ= 12.5 cm = 0.125 m
Volume of the container = 0.250 L = 250 mL
The density of water = 1 g/mL
Density = mass /volume
Mass = Volume × Density
Thus; the mass of the water = 250 mL × 1 g/mL
the mass of the water = 250 g
the specific heat of water s = 4.18 J/g° C
the initial temperature = 20.0° C
the final temperature = 99° C
Change in temperature = (99-20)° C = 79 ° C
The heat q absorbed during the process = ms
The heat q absorbed during the process = 250 g × 4.18 J/g° C × 79° C
The heat q absorbed during the process = 82555 J
The energy of a photon can be represented by the equation :
= hc/λ
where;
h = planck's constant =
c = velocity of light =
=
= J
The total photons required = Total heat energy/ Energy of a photon
The total photons required =
The total photons required = 5.19 × 10²⁸ photons