Why am I struggling with multiple choice exams in A level Chemistry?

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Struggling with multiple choice exams in A level Chemistry is a common issue, particularly with the Cambridge format that includes complex questions. A student reported scoring 82% overall but only 14/40 on the multiple choice section, despite excelling in structured theory questions. The discussion highlights the importance of practice and understanding the basics to improve performance on multiple choice exams. Strategies such as elimination and focused study on question types may help address the difficulties faced. Overall, consistent practice and refining test-taking strategies are essential for success in these challenging assessments.
prasannapakkiam
:frown:I just got the results from a mock exam that actually counts towards next year... I got 82%. However everyone else got 95+! It is the multichoice - I got 14/40 for it! The structured theory - I got 98%. Does anybody have any good sites or tips to combat this Multichoice problem I have? Also this is A level Chemistry conducted by Cambridge... So they have this 'multiple multi choice'. I just do not see why I get soo bad. Is it due to lack of study? or just lack of practice? :frown::frown:
 
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hello! friend the pattern also exists in IIT-JEE of india...we too have to make it out...the general strategy to solve multi's is to solve from the basics and to solve the " by-products" hand-by-hand..so to get a list of answerrs...
cheers!
 
Really? My cousins tell that once in IIT, it is a worry free life for them! But then again, they barely passed... But with the ambiguities in these MC questions, I just cannot do them in time! The same story goes for my Physics: Structured lim--> 100, multichoice lim-->0. So elimination and more study is probably the only way through them?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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