Which one of the following statements is true about the equilibrium constant for a reaction if δg° for the reaction is negative? k > 1 k < 1 k = 1 k = 0

Answer : K > 1is the true statement about the equilibrium constant for a reaction if for the reaction is negative.

Explanation :

The relation between the equilibrium constant and standard Gibbs, free energy is:

where,

= standard Gibbs, free energy

R = gas constant

T = temperature

K = equilibrium constant

From the above relation we conclude that,

When K > 1 then the value of is negative.

When K < 1 then the value of is positive.

When K = 1 then the value of is zero.

When K = 0 then the value of is undefined.

Hence, K > 1is the true statement about the equilibrium constant for a reaction if for the reaction is negative.

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol