Balancing Equations: Carbon Disulfide and Ammonia Reaction

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The discussion revolves around balancing the chemical equation for the reaction between carbon disulfide (CS2) and ammonia (NH3), which produces hydrogen sulfide (H2S) and ammonium thiocyanate (NH4NCS). The original attempt at balancing the equation was incorrect, as it mistakenly used C2S instead of the correct formula CS2 for carbon disulfide. Participants emphasize the importance of correctly identifying chemical formulas and balancing the number of atoms on each side of the equation. The correct balanced equation should reflect the stoichiometry of the reactants and products accurately. Proper understanding of chemical reactions is crucial for success in chemistry assignments.
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I can't seem to figure out a problem for my a/p chemistry summer assignment review. If you could help me that would be great.

The problem is: Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocuanate.

This is what my answer was but it is wrong and unbalanced.
C2S + NH3 = H2S + NH4NCS
 
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Carbon disulfide, sounds as CS2, not C2S...
 
Last edited:
thank you
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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