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Chemistry
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5 Jun 2020

In the following reaction, what is the concentration of H2 at equilibrium if there are 1.00 moles of Cl2 at equilibrium? There are 5.50 moles of H2 and 4.00 moles of Cl2 at the beginning of the reaction mixed in a 2.00 vessel container.

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General Chemistry 2
Skill
Relate equilibrium concentrations of reactants and products
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Hubert Koch
Hubert KochLv2
1 Sep 2020

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for the rection H2(g)+cl2(g) ....> 2Hcl(g) determine theequilbrium constant K0p.how many mole oh hclare forme if o.250 moles of H2 and 0.250moles of cl2 are mixed andbrought to equilibrium at 298 k in a 3 liter container?? How manymole of H2 and CL2 are in the equilibrium mixture? what is theconcentration (in mol/l) of each gas at eqilibrium? assume idealgas behavior

The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K.

PCl3(g) + Cl2(g) <-----> PCl5(g)

Calculate the equilibrium concentrations of reactant and products when 0.358 moles of PCl3 and 0.358 moles of Cl2 are introduced into a 1.00 L vessel at 500 K.

[PCl3] = ____ M
[Cl2] = ____ M
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Consider the reaction H2(g) + Cl2(g) → 2HCl(g)ΔH = −184.6 kJ / mol If 1.00 moles of H2 react with 1.00 moles of Cl2 to form HCl, what is ΔU (in kJ) for this reaction at 1.0 atm and 25°C? Assume the reaction goes to completion.

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