Given delta G of the reaction is -2870 kJ
We know that , if delta G is negative , reaction is spontaneous
Delta G = - RTlnK
-2870 *1000 =- 8.314*298*ln K
K >>>>>>1
Reaction will be spontaneous
Is the reaction C_6H_12O_6 + 6O_2 rightarrow 6CO_2 + 6H_2O (delta G^0 = -2870 kJ) spontaneous...
Glucose, C_6H_12O_6, is used as an energy source by the human body. The overall reaction in the body is described by the equation c_6H_12O_6 (aq) + 6O_2(g) rightarrow 6CO_2(g) + 6H_2O(t) Calculate the number of grams of oxygen required to convert 48.0 g of glucose is CO_2 andH_2O. 61.9 g O_2 Also compute the number of grams of CO_2 produced. 85.07 g CO_2
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both....
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...
What is Delta G in kJ for the reaction: Cl_2(g)+ 2 Br^- rightarrow Br_2(l) + 2 Cl^- if [Br^-] = 0.100, [Cl^-] = 0.50, and p(Cl_2) = 1.00 atm? The temperature 25 degree C.
Consider the following reaction: 2Ca(s) + O_2(g) rightarrow 2CaO(s) Delta H_rxn = -1269.8 kJ; Delta S_rxn degree = -364.6 J/K Assume that all reactants and products are in their standard states. Part A Calculate the free energy change for the reaction at 28 degree C. Part B Is the reaction spontaneous? spontaneous nonspontaneous
Physical chemistry question For the reaction: creatine phosphate + H2O rightarrow creatine + P_i, delta G degree = 37.6 kJ at 310 K will the above reaction proceed forwards or backwards when the initial concentrations are: [creatine phosphate] = 1.2 times 10^-7 M [creatine] = 7.8 times 10^-1 M [P_i] = 9.2 times 10^-1 M
Use the standard reaction enthalpies given below to determine Delta H_rxn degree for the following reaction: 2 S(s) + 3 O_2(g) rightarrow 2SO_3(g) Delta H_rxn degree Given: SO_2(g) rightarrow S(s) + O_2(g) Delta H_rxn degree = +296.8 kJ 2SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H_rxn degree = -197.8 kJ Name those compounds? Li_2SO_3 Al_2S_3 P_2O_3 COBr_2-6H_2O
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
Using the following reactions: N_2(g) + O_2(g) rightarrow 2 NO(g) Delta H = 181 kJ times 2 NO(g) + O_2 rightarrow 2 NO_2(g) Delta H = -113 kJ times 2 N_2O(g) rightarrow 2 N_2(g) + O_2(g) Delta H = -163 kJ times Determine the enthalpy change for the reaction: N_2O(g) + NO_2(g) rightarrow 3 NO(g) Delta H =
Find the delta G degree for the following reaction two ways. Is the reaction spontaneous? Also, calculate the thermodynamic equilibrium constant for the reaction. P_2(g) + 10 HCl(ai) rightarrow 2 PCl_5(g) + 5H_2(g)