Answer: it will take 89.93secs
Explanation:Please see attachment for explanation
DUE IN 30 MINUTES!!! (please keep it short if you can, if not its ok.) What is the molar mass of Pb(SO4)2? Explain how you calcu
2 answers:
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Answer:
See explaination
Explanation:
The invariant mass of an electron is approximately9. 109×10−31 kilograms, or5. 489×10−4 atomic mass units. On the basis of Einstein's principle of mass–energy equivalence, this mass corresponds to a rest energy of 0.511 MeV.
Check attachment for further solution to the exercise.
Mass of Oxygen: 0.0159 grams
Moles of Oxygen: 9.94x10^-4
To find the mass of oxygen, subtract the mass of copper from the total mass.
There are 0.0159 grams of Oxygen.
To find how many moles there are, divide the given amount of oxygen by the molar mass (atomic mass) of oxygen because that mass is the same as one mole of oxygen.
Molar mass of Oxygen: 16.00
There are 9.94*10^-4 moles of Oxygen.
The question is incomplete, here is the complete question:
Phosgene, , gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:
The value of for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which
and
?
<u>Answer:</u> The equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.
<u>Explanation:</u>
The relation of is given by:
= Equilibrium constant in terms of partial pressure
= Equilibrium constant in terms of concentration = 5.79
= Difference between gaseous moles on product side and reactant side =
R = Gas constant =
T = Temperature = 570 K
Putting values in above equation, we get:
We are given:
Initial partial pressure of CO = 0.265 atm
Initial partial pressure of chlorine gas = 0.265 atm
Initial partial pressure of phosgene = 0.00 atm
The given chemical equation follows:
<u>Initial:</u> 0.265 0.265
<u>At eqllm:</u> 0.265-x 0.265-x x
The expression of for above equation follows:
Putting values in above equation, we get:
Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure
So, the equilibrium partial pressure of CO =
The equilibrium partial pressure of
The equilibrium partial pressure of
Hence, the equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.