Question

In this reaction had an 85.0% yield, how much CH4 was produced from 1250g C

Answer 1

start by writing a balanced equation

Answer 2

but what is my equation going to contain if I have one compound?

Answer 3

@aaronq

Answer 4

oh wait 2C + 2H20 ---> CH4 + CO2 okay know what

Answer 5

hmm i would've done \(C + 2H_2 \rightarrow CH_4\)

Answer 6

so now you wanna convert the mass of C to moles, then find the moles of \(CH_4\) that can be produced with that much C.

Use the stoichiometric coefficients to find moles produced.
Set up a ratio using the species of interest, like so:

e.g. for a general reaction:

\(\color{red}{a}A + \color{blue}{b}B\) \(\rightleftharpoons\) \( \color{green}{c}C\)

where upper case are the species (A,B,C), and lower case (a,b,c) are the coefficients ,

\(\dfrac{n_A}{\color{red}{a}}=\dfrac{n_B}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\)

From here you can isolate what you need.
For example: if you have 2 moles of B, how many moles of C can you produce?

solve algebraically: \(\dfrac{2}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\rightarrow n_C=\dfrac{2*\color{green}{c}}{\color{blue}{b}}\)


Now, since they said you have an 85% yield, multiply the moles of CH4 you found by 0.85 to finish the question.