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anonymous
 4 years ago
Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.
anonymous
 4 years ago
Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0@TheMind @ujjwal @ajprincess

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

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

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

UnkleRhaukus
 4 years ago
Best ResponseYou've already chosen the best response.1can you balance the equation for number of H and N on each side?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0UR EQ IS NT APPEARING

UnkleRhaukus
 4 years ago
Best ResponseYou've already chosen the best response.1so to make the product we need thee time as much H as N

ujjwal
 4 years ago
Best 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!

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Is this always the case??

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0ITS AGAIN APPEARING MATHS PROCCESING ERROR

mayankdevnani
 4 years ago
Best ResponseYou've already chosen the best response.0i think ujjwal is right

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

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

UnkleRhaukus
 4 years ago
Best ResponseYou've already chosen the best response.1which is the limiting reagent ?

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

UnkleRhaukus
 4 years ago
Best ResponseYou've already chosen the best response.1so according to the balanced equation the theoretical yield will be 2 moles of NH_3

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

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

UnkleRhaukus
 4 years ago
Best ResponseYou've already chosen the best response.1can you finish @Ruchi. ?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0@mayank i'm nt getting u properly

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0@taylorrrr @ajprincess @imron07 @TheMind @Vikt0r hlp me out

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

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