Question

what is the value of δg when [h ] = 5.4×10−2m , [no−2] = 6.3×10−4m and [hno2] = 0.21 m ? express your answer using three significant figure.

Answer 1

To determine the value of ΔG, we need to use the equilibrium constant (K) which can be calculated using the concentrations of the reactants and products at equilibrium. Without the temperature, we cannot directly calculate ΔG, but we can use the equation ΔG = -RTln(K) once we have the value of K.

Step-by-step explanation:

The value of ΔG can be determined using the equation ΔG = -RTln(K), where R is the gas constant (8.314 J/mol·K) and T is the temperature in Kelvin. However, the temperature is not given in the question, so we cannot calculate ΔG directly.

To solve this problem, we need the equilibrium constant (K) for the reaction. The equilibrium constant can be calculated using the concentrations of the reactants and products at equilibrium. In this case, the concentrations given are [H], [NO-2], and [HNO2]. We can use these concentrations to calculate the value of K and then use that value to calculate ΔG.

First, we need to determine the concentrations of [H+], [NO2-], and [HNO2] using the values given in the question. Then, we can use these concentrations to calculate the value of K. Finally, we can use the value of K to calculate ΔG using the equation ΔG = -RTln(K).

Answer 2

Without the value of ΔG° and the temperature (T), it is not possible to calculate the Gibbs free energy change (ΔG) for the reaction. The necessary values must be obtained from additional resources such as the standard Gibbs free energy change table or course materials.

Step-by-step explanation:

To determine the value of ΔG (Gibbs free energy change) for the reaction involving H+, NO2−, and HNO2 at a given concentration, we can use the formula:

ΔG = ΔG° + RTlnQ

where ΔG° is the standard Gibbs free energy change, R is the universal gas constant, T is the temperature in Kelvin, and Q is the reaction quotient at a given moment.

However, without the value of ΔG° and the temperature (T), we cannot calculate ΔG. To find ΔG°, we would need to consult Table E1 for the standard Gibbs free energy change of the reaction involving HNO2. Additionally, we would need the temperature at which the reaction is occurring to use the universal gas constant (R).

Since we lack the necessary values of ΔG° and T to proceed with the calculation, we are unable to provide an answer to the question posed. To calculate ΔG, you will need to obtain these missing values from your course material or an established database.