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Ruchi.
Group Title
Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.
 one year ago
 one year ago
Ruchi. Group Title
Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.
 one year ago
 one year ago

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Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
@TheMind @ujjwal @ajprincess
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
have you got an equation for the reaction
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
do you know the for mula for ammonia?
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
is it NH_3 ?
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
so far we have \[N_2+H_2 \longrightarrow NH_3\] right?
 one year ago

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
@@@UnkleRhaukus
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
can you balance the equation for number of H and N on each side?
 one year ago

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
UR EQ IS NT APPEARING
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
N_2 + H_2 ⟶ NH_3
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
so to make the product we need thee time as much H as N
 one year ago

ujjwal Group TitleBest ResponseYou've already chosen the best response.0
\[N_2+3H_2\rightarrow2NH_3\] You get no of moles required from this equation! Convert them in terms of weight.. Find limiting reactant (the reactant whose quantity is less than required)! limiting reactant will determine the amount of product formed!
 one year ago

bthemesandtricks Group TitleBest ResponseYou've already chosen the best response.0
Is this always the case??
 one year ago

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
ITS AGAIN APPEARING MATHS PROCCESING ERROR
 one year ago

mayankdevnani Group TitleBest ResponseYou've already chosen the best response.0
i think ujjwal is right
 one year ago

mayankdevnani Group TitleBest ResponseYou've already chosen the best response.0
N2 + 3H2 > 2NH3
 one year ago

mayankdevnani Group TitleBest ResponseYou've already chosen the best response.0
So the moles are: For nitrogen, 28g/28g/mol = 1.0 mole N2 For hydrogen 25g/2g/mole = 12.5 moles @ujjwal right...
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
which is the limiting reagent ?
 one year ago

mayankdevnani Group TitleBest ResponseYou've already chosen the best response.0
Obviously, hydrogen is in excess and nitrogen is the limiting reagant
 one year ago

mayankdevnani Group TitleBest ResponseYou've already chosen the best response.0
@UnkleRhaukus
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
so according to the balanced equation the theoretical yield will be 2 moles of NH_3
 one year ago

ujjwal Group TitleBest ResponseYou've already chosen the best response.0
yep! 2 mol of NH3 will be yielded!
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
the molar mass of ammonia is (1x14+3x1) g/mol
 one year ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
can you finish @Ruchi. ?
 one year ago

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
@mayank i'm nt getting u properly
 one year ago

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
@taylorrrr @ajprincess @imron07 @TheMind @Vikt0r hlp me out
 one year ago

ajprincess Group TitleBest ResponseYou've already chosen the best response.0
Where are u stuck @Ruchi.?
 one year ago

ajprincess Group TitleBest ResponseYou've already chosen the best response.0
Did u understand the part where the moles are calculated?
 one year ago
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