1)The value of Kp for the reactionCO2 +C 2CO is 3 at 1000 K. If initially pCO2=0.48 bar and pCO=0bar and pure graphite is present, calculate the equilibrium partial pressure of CO and CO2.2) The ionization constant of HF is 3.2*10^(-4). Calculate the degree of dissociation of HF in its 0.02M solution. Calculate the concentration of all species present (H30+, F, HF) in the solution and its pH. Do we have to multiply the initial concentration of the reactant to the degree of dissociation of equilibrium concentration of reactant and product?

1)The value of Kp for the reactionCO2 +C 2CO is 3 at 1000 K. If initi

1.	1)The value of Kp for the reactionCO2 +C 2CO is 3 at 1000 K. If initially pCO2=0.48 bar and pCO=0bar and pure graphite is present, calculate the equilibrium partial pressure of CO and CO2.2) The ionization constant of HF is 3.2*10^(-4). Calculate the degree of dissociation of HF in its 0.02M solution. Calculate the concentration of all species present (H30+, F, HF) in the solution and its pH. Do we have to multiply the initial concentration of the reactant to the degree of dissociation of equilibrium concentration of reactant and product?
Answer» 1)The value of Kp for the reaction CO2 +C <=> 2CO is 3 at 1000 K. If initially pCO2=0.48 bar and pCO=0bar and pure graphite is present, calculate the equilibrium partial pressure of CO and CO2. 2) The ionization constant of HF is 3.2*10^(-4). Calculate the degree of dissociation of HF in its 0.02M solution. Calculate the concentration of all species present (H30+, F, HF) in the solution and its pH. Do we have to multiply the initial concentration of the reactant to the degree of dissociation of equilibrium concentration of reactant and product?