The vapor pressure of water changes with temperature, as shown here. T (°C) P (torr) 21 18.7 22 19.8 23 21.1 24 22.4 25 23.8 26 25.2 27 26.7 28 28.4 J Calculate the magnitude of the current in amperes if the number of moles of hydrogen gas produced is 5.13x10-4 mol (from part A). Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) O 0.471 PA A ?

The following reaction has a AG° value of +8.43 kJ/mol at 25 °C. HA(aq) + H20(1) =H;O*(aq) + A (aq) Calculate the KA for the acid HA.

The Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).

Calculate the Gibbs free energy

Determine the standard Gibbs free energy of reaction, in kJ/mole, for the reaction of aqueous sodium carbonate with hydrochloric acid. G values for the reactants and products are given below. NaCO(aq) + 2 HCl(aq)  2 NaCl(aq) + HO() + CO(g)  NaCO(aq) -1051.6HCl(aq) -131.2NaCl(aq) -393.1HO() -237.1CO(g) -394.4

please help me with part b. Keep getting wrong.,

For a certain chemical reaction, the equilibrium constant  K   =   ×7.7106  at  5.00   °C . Calculate the standard Gibbs free energy of reaction.Round your answer to  2  significant digits.

A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ

For a certain chemical reaction, the equilibrium constant K = 2.8 × 104 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = kJ x10 X Ś

Use the reactions and AG° values below to determine AG° for: 3 CH4(g) + 4 O2(g) → C302(g) + 6 H20(g) For CH4(g) + 2 O2(g) → CO2(g) + 2 H20(g) For 3 CO2(g) → C302(g) + 2 O2(g) AG° = -800.8 kJ/mol AG° = +1073.4 kJ/mol %3D 272.6 kJ/mol 817.8 kJ/mol None of the answers are correct -345.8 kJ/mol -1329.0 kJ/mol