# Basic equilibrium problem

1. I am having trouble figuring out how to work the most basic equilibrium problem when there is an initial concentration of reactants only and no product. How am I supposed to find the constant with a zero in my quotient? Here is an example problem:
At 527˚C, K = 0.0160 for the following reaction: 2HI(g) ↔ H2 (g) + I2 (g)
What is the equilibrium concentration of H2
if the initial concentrations of both H2 and I2
= 0.0160 M and the initial concentration of
HI = 0 M?

2. k = product/reactant

3. If I knew where to start I wouldn't need help

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1. I am having trouble figuring out how to work the most basic equilibrium problem when there is an initial concentration of reactants only and no product. How am I supposed to find the constant with a zero in my quotient? Here is an example problem:
At 527˚C, K = 0.0160 for the following reaction: 2HI(g) ↔ H2 (g) + I2 (g)
What is the equilibrium concentration of H2
if the initial concentrations of both H2 and I2
= 0.0160 M and the initial concentration of
HI = 0 M?

2. k = product/reactant

3. If I knew where to start I wouldn't need help
You mentioned that K=[product]/[reactants] - write this equation out in full detail and remember that they refer to the equilibrium values.

one way of solving this problem is by breaking it into parts.

initially,