If 42.5 g of CH4 and 75.9 g of S8 react, how many grams of H2S are produced? 2 CH4(g) + S8(g) 2 CS2(g) + 4 H2S(g)
Added by Jacob W.
Step 1
Given: Mass of CH4 = 42.5 g Molar mass of CH4 = 16 g/mol Number of moles of CH4 = Mass/Molar mass Number of moles of CH4 = 42.5 g / 16 g/mol Number of moles of CH4 ≈ 2.66 mol Show more…
Show all steps
Your feedback will help us improve your experience
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
If 7.1 g of CH4 and 5.5 g of S react, what is the mass, in grams, of H2S that is produced? CH4(g) + 4S(g) ?CS2(g) + 2H2S(g)
Bobby B.
How many grams of CH4 are produced when 112 g Al4C3 react with 174 g H2O?
Adi S.
When 20.5 g of methane and 45.0 g of chlorine gas undergo a reaction that has a 75.0$\%$ yield, what mass (g) of chloromethane $\left(\mathrm{CH}_{3} \mathrm{Cl}\right)$ forms? Hydrogen chloride also forms.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD