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For a certain chemical reaction, the standard Gibbs free energy of reaction is 72.4 kJ. Calculate...
For a certain chemical reaction, the standard Gibbs free energy of reaction is −141. kJ. Calculate the temperature at which the equilibrium constant K=3.6 x 10^25.
For a certain chemical reaction, the standard Gibbs free energy of reaction at 25.0 °C is − 84.7 kJ . Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
For a certain chemical reaction, the standard Gibbs free energy of reaction at 10.0 °C is 99.8 kJ. Calculate the equilibrium constant for this reaction. Round your answer to 2 significant digits. K = 0 x 5 ?
Question 2 For a certain chemical reaction, the standard Gibbs free energy of reaction at 25.0°C is 126.kJ. Calculate the equilibrium constant K for this reaction.Round your answer to 2 significant digits.
estion For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is 84.2 kJ . Calculate the equilibrium constant K for this reaction.
I cannot seem to figure it out. The standard Gibbs-free energy of a system is related to its equilibrium constant through the following equation. AG = R.T.In(K) In this equation R is the gas constant, T is the temperature, and the next to AG defines the conditions as standard ambient temperature and pressure, i.e. "SATP". (Answer the following questions to three significant figures.) (a) Given an equilibrium constant of 6.28 x 10-3, what is its standard Gibbs-free energy? 4.9 12.6...
3. + 2.5/10 points Previous Answers McM8 6.P.012. The standard Gibbs-free energy of a system is related to its equilibrium constant through the following equation. AG° = -R·T· In(K) In this equation R is the gas constant, T is the temperature, and the ° next to AG defines the conditions as standard ambient temperature and pressure, i.e. "SATP". (Answer the following questions to three significant figures.) (a) Given an equilibrium constant of 4.53 x 10-6, what is its standard Gibbs-free...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Calculate the change in Gibbs free energy at standard conditions (TSS) and the equilibrium constant for each of the following reactions. (a) CH4(g) + H2O(g) equilibrium reaction arrow CO(g) + 3 H2(g); ?H° = +205.9 kJ, ?S° = +214.7 J/K ?G° 141.9 Correct: Your answer is correct. kJ K (b) CaCO3(s) equilibrium reaction arrow CaO(s) + CO2(g); ?H° = +179.2 kJ, ?S° = +160.2 J/K ?G° 131.5 Correct: Your answer is correct. kJ K
If you find that the standard Gibbs free energy change for a reaction is -6.56 kJ/molk, what is the equilibrium constant for the reaction at 25.0 °C? Be careful with your units in the calculation. For a reaction, a plot of In K versus inverse temperature is found to be linear and fits the following equation: y = -1,838x + 6.81. What is the value of AH? Give your answer with units of kJ/molk; however, you should not type in...