We have a solution that has a concentration of 0.362 M for A(aq) and 0.650 M for B(aq). There are no other solutes initially. The reaction 2 A(aq) + B(aq) <---> 2 C(aq) + D(aq) takes place. At equilibrium, the concentration of C(aq) is 0.127 M. What is the equilibrium constant of this reaction?
For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.64 kJ at 25oC. The initial concentration of A(aq) is 0.555 M, the initial concentration of B(aq) is 0.301 M, and the initial concentration of C(aq) is 0.243 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25oC)?
We start with a pure sample of A(g). The following equilibrium is established:
2 A(g) <---> B(g) + C(g)
The total pressure is 8.40 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.06 atm. Calculate the value of the standard Gibbs free enthalphy change (in kJ) for this reaction at 25.0oC.
What volume (in mL) of a solution 0.160 M in Ca(OH)2 must we use to neutralize 29.0 mL of a solution 0.337 M in H3PO4.
We have 2.82 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 8.94 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution?
What is the pH of a 0.100 M solution of the acid HA if its ionization constant, KA, is 0.32 .
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