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X is a mixture of two compounds of Group II elements. X can undergo thermal decomposition to produce a white solid and only two gaseous products. One of the gaseous products relights a glowing splint. What could be the components of mixture X?
A MgCl 2 and CaCO3
B MgCO3 and Ca(NO3)2
C Mg(NO3)2 and Ca(NO3)2
D MgO and CaSO4
the answer is C... how can you distinguish between all the options and conclude that C is the right one? i suck at periodicity... any advice?
View attachment 52141
Answer is B
View attachment 52142
Answer is A
Why? Why not C since the forward reaction is exothermic increasing temperature would the favour the reactants side right?
Equilibrium means that the rate of forward reaction is equal to the rate of backward reaction.Increasing the temperature will increase the rates of both the forward and backward reactions, it's just that the backward reaction will increase at a faster rate.
Remember, the reaction is in equilibrium.
Equilibrium has to be dynamic, in that, both the forward and backward reactions must be equal. If you only have one increasing, there will be an imbalance and so no equilibrium would exist.
View attachment 52145
How would I solve this? ,_,
Equilibrium means that the rate of forward reaction is equal to the rate of backward reaction.
So they increased the temperature and still want it to be in Equilibrium?
When the temperature is increased the temperature more of products will be formed since forward reaction is exothermic....but since they want equilibrium both sides increase...
Did I get it right ?
Why are BOTH increasing?Both will increase, just one increases faster than the other to produce the yield faster.
View attachment 52146
Answer is C
You already said why, because you still want the reaction to be in equilibrium.Why are BOTH increasing?
Thank you for your help!
Yes...okayYou already said why, because you still want the reaction to be in equilibrium.
was rightEquilibrium means that the rate of forward reaction is equal to the rate of backward reaction.
So they increased the temperature and still want it to be in Equilibrium?
When the temperature is increased the temperature more of products will be formed since forward reaction is exothermic....but since they want equilibrium both sides increase...
Did I get it right ?
View attachment 52149
Can someone please answer this question for ME PLEASEEEEEEEEEEEEEEE AND EXPLAINN THANKYOU
ANSWER IS B BUT YYYYYYYYYYYYYe
You write out the bromination of propane.
Br2 ---> 2Br・
Br・ + C3H8 ---> C3H7・ + HBr
C3H7・ + Br2 ----> C3H7Br + Br・
Br・ + C3H8 ----> C3H7 ・ + HBr
Then in the termination step, you have two radicals react. So you can have C3H7・ and C3H7・ react to form C6H14.
The catch here is that there's two types of radicals that react. It may look like it's just C3H7・, but the ・ can be attached to 2 different carbons in C3H7. Either the first or the second.
Like so,
CH3CH2CH2・
Or
CH3CH・CH3
Option 1 follows,
CH3CH2CH2・ + CH3CH・CH3
While option 2 follows,
CH3CH・CH3 + CH3CH・CH3
Option 3 cannot be formed because no combination of CH3CH・CH3 and CH3CH2CH2・ would allow for it.
Hope that made sense!
im so weak in this . do u have an easy explaination ? i understood the radical part but applying it was difficult.
thanks really for the tip
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