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Answer:
Mass of carbon = 109.1 g
Explanation:
Given data:
Mass of carbondioxide = 400 g
Mass of carbon = ?
Solution:
Molar mass of carbon = 12 g/mol
Molar mass of CO₂ = 44 g/mol
Mass of carbon in 400g of CO₂:
Mass of carbon = 12 g/mol/44 g/mol × 400 g
Mass of carbon = 109.1 g
Use the formula for second order reaction:

C = concentration at time t
C0 = initial conc.
k = rate constant
t = time
1st equation :

2nd Equation:

Find

from 1st equation and put it in 2nd equation:


k = 0.046
There are 1.2 hr would this current have to be applied to plate out 7. 20 g of iron .
Calculation ,
Given ; Current ( I ) = 5. 68 A
In
, the valancy of Fe is +2 .
2 moles of
are required for the decomposition of 1 mole of Fe .
7. 20 g of Fe in moles = 7. 20 g /55.845 g/mol =0.12 mole
x moles of
are required for the decomposition of 0.128 mole of Fe .
moles of
are required = 0.256 moles
Charge on 1 mole of
= 96500 C
Charge on 0.256 mole of
= 24704 C
Current ( I )= Q/t
t =Q / I = 24704 C/5. 68 A = 4349 sec = 1.2 hr
Therefore , there are 1.2 hr would this current have to be applied to plate out 7. 20 g of iron .
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Answer: Option (B) is the correct answer.
Explanation:
As the given reaction is as follows.
Equilibrium constant for this reaction will be as follows.
![K_{c} = \frac{[CO_{2}]}{[CO]^{2}}](https://tex.z-dn.net/?f=K_%7Bc%7D%20%3D%20%5Cfrac%7B%5BCO_%7B2%7D%5D%7D%7B%5BCO%5D%5E%7B2%7D%7D)
According to Le Chatelier's principle, when we increase the temperature then the equilibrium will shift towards the right hand side.
As a result, concentration of carbon dioxide will decrease whereas concentration of carbon monoxide will increase.
Thus, we can conclude that in the given reaction equilibrium constant for this reaction will decrease with increasing temperature.