Question

I need help with 11th grade chemistry, I will put a picture in.

Answer 1

hi

Answer 2

Sorry my handwriting was bad my friend kept moving my hand

Answer 3

it is okay, I am trying to figure it out rn

Answer 4

Oh thank you!

Answer 5

For B, the limiting reactant is O2 because you need more moles of O2 in the original equation

Answer 6

Thank you

Answer 7

for D the equation is % yield = (actual amount produced / theoretical amount) x 100

Answer 8

How do i find those out?

Answer 9

the theoretical yield is the molar mass of the whole thing

Answer 10

and the actual amount is what the problem gives you

Answer 11

so (137.1 g / 149 g) x 100 = 91.8 % yield

Answer 12

Ok i that is the equation? Now i have to solve it

Answer 13

yes, I solved it for you, but double check

Answer 14

Ok

Answer 15

8.3 moles H2S x (2 moles H2O / 2 moles H2S) = 8.3 moles H2O = theoretical amount produced

Answer 16

sorry you were confused! this is C above ^^ (thought I posted it already but I didn't...)

Answer 17

So i find the molar mass of the whole equation or just one side?

Answer 18

a medal and fan is appreciated!

Answer 19

haha yes i was

Answer 20

agreed @ master

Answer 21

just do exactly what I told you

Answer 22

nice job @ master

Answer 23

thanks haha @SyedMohammed98

Answer 24

You're Welcome :)