Using the equation below, calculate the percent yield of H3PO4 if an experiment that started with 12.98 grams of HCl and excess
1 answer:
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Answer: The new partial pressures of when equilibrium is re-established are 223.4 torr, 6.82 torr and 26.4 torr respectively.
Explanation:
For the given chemical reaction:
The expression of for above reaction follows:
........(1)
We are given:
Putting values in above equation, we get:
Now we have to calculate the new partial pressure of .
The reaction is re-established and proceed to right direction by Le-Chatelier's principle to cancel the effect of addition of .
Now, the equilibrium is shifting to the reactant side. The equation follows:
Initial: 13.2 32.8 217.0
At eqm: 13.2-x 32.8-x 217.0+x
Putting values in expression 1, we get:
Neglecting the 40.4 value of 'x' because pressure can not be more than initial partial pressure.
Thus, the value of 'x' will be, 6.38 torr.
Now we have to calculate the new partial pressures after equilibrium is reestablished.
Partial pressure of = (217.0+x) = (217.0+6.38) = 223.4 torr
Partial pressure of = (13.2-x) = (13.2-6.38) = 6.82 torr
Partial pressure of = (32.8-x) = (32.8-6.38) = 26.4 torr
Hence, the new partial pressures of when equilibrium is re-established are 223.4 torr, 6.82 torr and 26.4 torr respectively.
Answer:
The maximum wavelength of light for which a carbon-hydrogen single bond could be broken by absorbing a single photon = 290 nm
Explanation:
So to break a single C - H bond require =
= 6.84 x 10⁻¹⁹ joule
Find the wavelength of a photon we use E = hν
⇒ E =
Where h = Planck's constant = 6.626 x 10⁻³⁴ J.K⁻¹.Mole⁻¹
c = speed of light = 3 x 10⁸ m/sec
Wavelength =
= 2.9 x 10⁻⁷ m
= 290 nm
∵ 1 nm = 10⁻⁹ m