How do you do this 1 mark a level chemistry question???
A research chemist investigates how to improve the synthesis of ethyne from methane at a high temperature. • The chemist adds CH4 to a 4.00 dm3 container. • The chemist heats the container and allows equilibrium to be reached at constant temperature. The total gas volume does not change. • The equilibrium mixture contains 9.36 × 10–2 mol CH4 and 0.168 mol C2H2.
(i) Calculate the amount, in mol, of H2 in the equilibrium mixture.
(i) Calculate the amount, in mol, of H2 in the equilibrium mixture.
In case you're still looking for an answer to this:
You start by writing out the balanced equation: 2CH4 <=> C2H2 + 3H2
Then you can use an initial-change-equilibrium table (they were called RICE tables at my school?) to figure out how much H2 you'd have by finding the difference between initial and final moles of ethyne
does that help?
You start by writing out the balanced equation: 2CH4 <=> C2H2 + 3H2
Then you can use an initial-change-equilibrium table (they were called RICE tables at my school?) to figure out how much H2 you'd have by finding the difference between initial and final moles of ethyne
does that help?
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