Ruchi.
Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.
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Ruchi.
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@TheMind @ujjwal @ajprincess
UnkleRhaukus
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have you got an equation for the reaction
Ruchi.
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no
UnkleRhaukus
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do you know the for mula for ammonia?
UnkleRhaukus
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is it NH_3 ?
Ruchi.
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nh3
UnkleRhaukus
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so far we have
\[N_2+H_2 \longrightarrow NH_3\]
right?
Ruchi.
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@@@UnkleRhaukus
UnkleRhaukus
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can you balance the equation for number of H and N on each side?
Ruchi.
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UR EQ IS NT APPEARING
UnkleRhaukus
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oh,
UnkleRhaukus
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N_2 + H_2 ⟶ NH_3
UnkleRhaukus
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so to make the product we need thee time as much H as N
ujjwal
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\[N_2+3H_2\rightarrow2NH_3\]
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!
bthemesandtricks
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Is this always the case??
Ruchi.
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ITS AGAIN APPEARING MATHS PROCCESING ERROR
mayankdevnani
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i think ujjwal is right
mayankdevnani
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N2 + 3H2 ---> 2NH3
mayankdevnani
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So the moles are:
For nitrogen, 28g/28g/mol = 1.0 mole N2
For hydrogen 25g/2g/mole = 12.5 moles
@ujjwal right...
UnkleRhaukus
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which is the limiting reagent ?
mayankdevnani
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Obviously, hydrogen is in excess and nitrogen is the limiting reagant
mayankdevnani
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@UnkleRhaukus
UnkleRhaukus
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so according to the balanced equation the theoretical yield will be 2 moles of NH_3
ujjwal
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yep! 2 mol of NH3 will be yielded!
UnkleRhaukus
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the molar mass of ammonia is (1x14+3x1) g/mol
UnkleRhaukus
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can you finish @Ruchi. ?
Ruchi.
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@mayank i'm nt getting u properly
Ruchi.
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@taylorrrr @ajprincess @imron07 @TheMind @Vikt0r hlp me out
ajprincess
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Where are u stuck @Ruchi.?
ajprincess
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Did u understand the part where the moles are calculated?