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

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

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

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

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

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

Ruchi. Group TitleBest ResponseYou've already chosen the best response.0
@@@UnkleRhaukus
 2 years 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?
 2 years ago

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

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
N_2 + H_2 ⟶ NH_3
 2 years 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
 2 years 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!
 2 years ago

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

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

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

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

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

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

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

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

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

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

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

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

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

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