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Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) +...
Calculate Delta G degree for the following reaction at 25 degree C: 3Zn^2+ (aq) + 2Al(s)...
Calculate Delta G degree for the following reaction at 25 degree C: 3Zn^2+ (aq) + 2Al(s) 3Zn(s) + 2Al^3+ (aq)
Balance the equation for the reaction observed: _ Cu(s) + HNO3(aq) → Cu(NO3)2(aq) +_ NO2(g) + H2O(1) 3. Add 40 mL...
Balance the equation for the reaction observed: _ Cu(s) + HNO3(aq) → Cu(NO3)2(aq) +_ NO2(g) + H2O(1) 3. Add 40 mL of 3.0 M NaOH (sodium hydroxide) to the solution in your beaker. Write the balanced equation for the reaction observed: 4. Add 2-3 boiling chips to your beaker and carefully heat the solution, while stirring with a stirring rod, just to the boiling point. (Do NOT boil. Have a low flame and keep the beaker well above the flame.)...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g),...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g), Delta G degree = -31.0 kJ consider the galvanic cell that uses the reaction 2 Ag^+ (aq) plus Cu(s) rightarrow Cu^2+ (aq) + 2Ag (s) clearly sketch the experimental set-up, write down the anode and cathode half- give the shorthand notation for the cell For the following cell, write a balanced equation for the cell reaction and calc Delta G degree C: Pt(s) |H_2(1.0...
Find the equilibrium concentration of N_2O_4(g) [Nitrogen nitroxide] due to the chemical reaction at 25 degree...
Find the equilibrium concentration of N_2O_4(g) [Nitrogen nitroxide] due to the chemical reaction at 25 degree C and 1 atm. N_2O_4(g) doubleheadarrow 2NO_2(g) Using the available data: (a) N_2O_4 (g) doubleheadarrow N_2(g) + 2O_2 (g), Delta G degree_rxn, 1 = Delta G degree_f, N_2O_4 = -23.41 kcal/mol (b) 0.5N_2(g) + O_2(g) doubleheadarrow NO_2(g), Delta G degree_rxn, 2 = -Delta G degree_f, NO_2 = -12.24kcal/mol
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g)...
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g) rightarrow Cl_2O (g)+ F_2O (g) Delta H_rxn^degree = 167.4 kJ/mol 2ClF_3 (g) +2O_2 (g) rightarrow Cl_2O (g) + 3F_2O (g) Delta H_rxn^degree = 341.4 kJ/mol 2F_2 (g) + O_2 (g) rightarrow 2F_2O (g) Delta H_rxn^degree = -43.4 kJ/mol At the same temperature, use Hess' law to calculate Delta H_rxn^degree for the following reaction: ClF (g) + F_2 (g) rightarrow ClF_3 (g)
Can someone help me finish my table? all the inforamtion is there. molarity of HCL =0.5M g...
can someone help me finish my
table? all the inforamtion is there.
molarity of HCL =0.5M
grams of borax = 18.41g
the Relationship between Thermodynamics and Equilibrium 21 Complete the data table for each temperature studied. Beaker Label 42 °C 45 °C 36 ° C 39 °C 33 °C 2EC 138℃-2°C| ーでー 46℃ Temperature reading (C) Absolute temperature (K) 1/T Final buret reading Initial buret reading Volume of HCI Moles of H+ Moles of B Os(OH)2 Molarity of B,Os(OH)2 306.230.2...
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of...
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of K_p and K_c at 25 degree C for the equilibrium: H_2O (l) H_2O(g). Vinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH_3COOH(aq) H^+(aq) + CH_3CO^-_2 (aq) a) Write the equilibrium constant expression for K_c. b) What is the value of K_c if the extent of dissociation of 1.0 M CH_3COOH is 0.42%? Determination of an Equilibrium Constant
Consider the following reaction which is at equilibrium at 25 degree C: NH_4(NH_2CO_2)(s) 2 NH_3(g) +...
Consider the following reaction which is at equilibrium at 25 degree C: NH_4(NH_2CO_2)(s) 2 NH_3(g) + CO_2(g), delta H degree = 152.2 kJ In which direction will the reaction shift if? *(a) the pressure is increased (b) the pressure decreased (c) the temperature is increased (d) the temperature is decreased (e) some CO_2 is added (f) NH_3 is removed (g) a catalyst is added (h) some NH_4(NH_2CO_2) is added (i) some Ne is added; and, (j) the volume is increased
In a study of the decomposition of nitramide in aqueous solution at 25 degree C NH_2NO_2(aq)...
In a study of the decomposition of nitramide in aqueous solution at 25 degree C NH_2NO_2(aq) rightarrow N_2O(g) + H_2O(1) the concentration of NH_2NO_2 was followed as a function of time. It was found that a graph of ln[NH_2NO_2] versus time in seconds gave a straight line with a slope of -6.72 times 10^-5 s^-1 and a y-intercept of -0.863. Based on this plot, the reaction is order in NH_2NO_2 and the rate constant for the reaction is s^-1.
Consider the following Gibbs energies at 25 degree C. Calculate Delta G degree _rxn for the...
Consider the following Gibbs energies at 25 degree C. Calculate Delta G degree _rxn for the dissolution of AgCl(s). Calculate the solubility-product constant of AgCl. K = Calculate Delta G degree_rxn for the dissolution of AgBr(s). Calculate the solubility-product constant of AgBr. K =
Calculate Delta G degree for the following reaction at 25 degree C: 3Zn^2+ (aq) + 2Al(s) 3Zn(s) + 2Al^3+ (aq)
Balance the equation for the reaction observed: _ Cu(s) + HNO3(aq) → Cu(NO3)2(aq) +_ NO2(g) + H2O(1) 3. Add 40 mL of 3.0 M NaOH (sodium hydroxide) to the solution in your beaker. Write the balanced equation for the reaction observed: 4. Add 2-3 boiling chips to your beaker and carefully heat the solution, while stirring with a stirring rod, just to the boiling point. (Do NOT boil. Have a low flame and keep the beaker well above the flame.)...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g), Delta G degree = -31.0 kJ consider the galvanic cell that uses the reaction 2 Ag^+ (aq) plus Cu(s) rightarrow Cu^2+ (aq) + 2Ag (s) clearly sketch the experimental set-up, write down the anode and cathode half- give the shorthand notation for the cell For the following cell, write a balanced equation for the cell reaction and calc Delta G degree C: Pt(s) |H_2(1.0...
Find the equilibrium concentration of N_2O_4(g) [Nitrogen nitroxide] due to the chemical reaction at 25 degree C and 1 atm. N_2O_4(g) doubleheadarrow 2NO_2(g) Using the available data: (a) N_2O_4 (g) doubleheadarrow N_2(g) + 2O_2 (g), Delta G degree_rxn, 1 = Delta G degree_f, N_2O_4 = -23.41 kcal/mol (b) 0.5N_2(g) + O_2(g) doubleheadarrow NO_2(g), Delta G degree_rxn, 2 = -Delta G degree_f, NO_2 = -12.24kcal/mol
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g) rightarrow Cl_2O (g)+ F_2O (g) Delta H_rxn^degree = 167.4 kJ/mol 2ClF_3 (g) +2O_2 (g) rightarrow Cl_2O (g) + 3F_2O (g) Delta H_rxn^degree = 341.4 kJ/mol 2F_2 (g) + O_2 (g) rightarrow 2F_2O (g) Delta H_rxn^degree = -43.4 kJ/mol At the same temperature, use Hess' law to calculate Delta H_rxn^degree for the following reaction: ClF (g) + F_2 (g) rightarrow ClF_3 (g)
can someone help me finish my
table? all the inforamtion is there.
molarity of HCL =0.5M
grams of borax = 18.41g
the Relationship between Thermodynamics and Equilibrium 21 Complete the data table for each temperature studied. Beaker Label 42 °C 45 °C 36 ° C 39 °C 33 °C 2EC 138℃-2°C| ーでー 46℃ Temperature reading (C) Absolute temperature (K) 1/T Final buret reading Initial buret reading Volume of HCI Moles of H+ Moles of B Os(OH)2 Molarity of B,Os(OH)2 306.230.2...
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of K_p and K_c at 25 degree C for the equilibrium: H_2O (l) H_2O(g). Vinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH_3COOH(aq) H^+(aq) + CH_3CO^-_2 (aq) a) Write the equilibrium constant expression for K_c. b) What is the value of K_c if the extent of dissociation of 1.0 M CH_3COOH is 0.42%? Determination of an Equilibrium Constant
Consider the following reaction which is at equilibrium at 25 degree C: NH_4(NH_2CO_2)(s) 2 NH_3(g) + CO_2(g), delta H degree = 152.2 kJ In which direction will the reaction shift if? *(a) the pressure is increased (b) the pressure decreased (c) the temperature is increased (d) the temperature is decreased (e) some CO_2 is added (f) NH_3 is removed (g) a catalyst is added (h) some NH_4(NH_2CO_2) is added (i) some Ne is added; and, (j) the volume is increased
In a study of the decomposition of nitramide in aqueous solution at 25 degree C NH_2NO_2(aq) rightarrow N_2O(g) + H_2O(1) the concentration of NH_2NO_2 was followed as a function of time. It was found that a graph of ln[NH_2NO_2] versus time in seconds gave a straight line with a slope of -6.72 times 10^-5 s^-1 and a y-intercept of -0.863. Based on this plot, the reaction is order in NH_2NO_2 and the rate constant for the reaction is s^-1.
Consider the following Gibbs energies at 25 degree C. Calculate Delta G degree _rxn for the dissolution of AgCl(s). Calculate the solubility-product constant of AgCl. K = Calculate Delta G degree_rxn for the dissolution of AgBr(s). Calculate the solubility-product constant of AgBr. K =
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