A sealed tube initially contains 9.84x10-4mol of H2and 1.38x10-3mol of I2. It is kept at 350C...
A sealed tube initially contains 9.84x10-4mol of H2and 1.38x10-3mol of I2. It is kept at 350C until the reaction H2(g) + I2(g) <=> 2HI (g) comes to equilibrium. At equilibrium 4.73x10-4moles of I2 are present. Calculate the number of moles of H2 and HI at equilibrium and the equilibrium constant Kc for the reaction.
(please provide steps on how to approach this problem) I noticed that the system is not initially at equilibrium so i used ICE method to find the values for the reactants and the products according to their ratio but it didn't work. For instance, I thought that because I2 is given at equilibrium(4.73x10^-4) then C for I2 in the ICE method would give me -1.853x10^-4 which indicates that the reactant lost that quantity. Then because I2 and H2 are 1:1 ratio then H2 also lost -1.853x10^-4. Please explain?
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A sealed tube initially contains 9.84x10-4mol of H2and
1.38x10-3mol of I2. It is kept at 350C...
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The following reaction was performed in a sealed vessel at 774 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...
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The following reaction was performed in a sealed vessel at 777 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...
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