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The c_p,m values of various real substances can be fit to the following equation, where a,...
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ...
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 =...
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...
4.20 If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15...
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
All four please thank you Which of the following is necessary for a process to be...
All four please thank you
Which of the following is necessary for a process to be spontaneous? A) Delta H_sys < 0 B) Delta S_sys > 0 C) Delta S < 0 D) Delta S_univ > 0 E) Delta G_sys = 0 Which reaction has the largest Delta S degree? A) 2 N_2H_4(g) rightarrow 2 NH_3(g) + H_2(g) B) O_2(g) + 2 H_2(g) rightarrow 2 H_2O(l) C) O_2(g) + 2 H_2(g) rightarrow 2H_2O(g) D) N_2(g) + 3H_2(g) rightarrow 2NH_3(g) E)...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3,...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3, 40 a 298 K. What is Delta G^Compositefunction for the following equilibrium? HA (aq) + H_2O(l) rightarrow leftarrow H_2O(aq) = A(aq) A) 7.95 kJ B) 30.8 kJ C) 11.4 kJ D) 19.4 kJ For a reversible phase change at constant temperature and pressure. A) Delta U = 0. B) Delta H = 0. C) w = 0 D) q = 0 E) Delta G...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree = -1408.4 kJ Calculate the following quantities. Find standard entropy values
Given rms speed, c = (3 RT/M)^1/2 Determine the temperature and pressure of 3.01 times 10^23...
Given rms speed, c = (3 RT/M)^1/2 Determine the temperature and pressure of 3.01 times 10^23 gas molecules, each with a mass of 6.64 times 10^-26 kg, in a 5 times 10^-3 m^3 container if the rms speed is 560 m/s. These molecules are distributed in 2 states with energies of 0 and 5 epsilon (epsilon =1.381 times 10^-21 J). There is no degeneracy for the first level. The second level is doubly degenerated. Calculate number of molecules in each...
Use Delta_fus H = 6.01 kJ/mol at 0 degree C for the sold rightarrow liquid phase...
Use Delta_fus H = 6.01 kJ/mol at 0 degree C for the sold rightarrow liquid phase transition of water to calculate Delta_fus S. The Calculated answer is J/mol K (1 decimal place.) The solubility of thallium chloride (TlCl) in water is 0.29 g in 100. mL of solution at 15.6 degree C. The molar concentration of Ti^+ is M (4 dec places). The molar concentration of Cl^- is M(1 dec places). The K_sp for TlCl at this temperature is (1...
(a) A muscle can be thought of as a fuel cell, producing work from the metabolism...
(a) A muscle can be thought of as a fuel cell, producing work from the metabolism of glucose (C6H1206): C6H1206 (glucose) +202(9) + 2H2O(l) + CO2(g). (0.1) Here g and I refer to the gaseous and liquid states, respectively. Using data given in the table, please determine the values of AH and AG for this reaction for one mole of glucose, assuming that the reaction takes place at room temperature and atmospheric pressure. Substance CH 20. (glucose) 0 (9) H200...
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ...
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ mol−1) CO2(g)CO2(g) −393.5−393.5 Ca(OH)2(s)Ca(OH)2(s) −986.1−986.1 H2O(l)H2O(l) −285.8−285.8 CaCO3(s)CaCO3(s) −1207−1207 H2O(g)H2O(g) −241.8−241.8 Part A: Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) C a ( O H ) 2 ( s ) + C O 2 ( g ) → C a C O 3 ( s ) + H 2 O ( l ) Express your answer in kJ mol−1 k J m o l...
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 =...
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...
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
All four please thank you
Which of the following is necessary for a process to be spontaneous? A) Delta H_sys < 0 B) Delta S_sys > 0 C) Delta S < 0 D) Delta S_univ > 0 E) Delta G_sys = 0 Which reaction has the largest Delta S degree? A) 2 N_2H_4(g) rightarrow 2 NH_3(g) + H_2(g) B) O_2(g) + 2 H_2(g) rightarrow 2 H_2O(l) C) O_2(g) + 2 H_2(g) rightarrow 2H_2O(g) D) N_2(g) + 3H_2(g) rightarrow 2NH_3(g) E)...
A 0.0403 M solution of a particular monoprotic weak acid. HA, has a pH of 3, 40 a 298 K. What is Delta G^Compositefunction for the following equilibrium? HA (aq) + H_2O(l) rightarrow leftarrow H_2O(aq) = A(aq) A) 7.95 kJ B) 30.8 kJ C) 11.4 kJ D) 19.4 kJ For a reversible phase change at constant temperature and pressure. A) Delta U = 0. B) Delta H = 0. C) w = 0 D) q = 0 E) Delta G...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree = -1408.4 kJ Calculate the following quantities. Find standard entropy values
Given rms speed, c = (3 RT/M)^1/2 Determine the temperature and pressure of 3.01 times 10^23 gas molecules, each with a mass of 6.64 times 10^-26 kg, in a 5 times 10^-3 m^3 container if the rms speed is 560 m/s. These molecules are distributed in 2 states with energies of 0 and 5 epsilon (epsilon =1.381 times 10^-21 J). There is no degeneracy for the first level. The second level is doubly degenerated. Calculate number of molecules in each...
Use Delta_fus H = 6.01 kJ/mol at 0 degree C for the sold rightarrow liquid phase transition of water to calculate Delta_fus S. The Calculated answer is J/mol K (1 decimal place.) The solubility of thallium chloride (TlCl) in water is 0.29 g in 100. mL of solution at 15.6 degree C. The molar concentration of Ti^+ is M (4 dec places). The molar concentration of Cl^- is M(1 dec places). The K_sp for TlCl at this temperature is (1...
(a) A muscle can be thought of as a fuel cell, producing work from the metabolism of glucose (C6H1206): C6H1206 (glucose) +202(9) + 2H2O(l) + CO2(g). (0.1) Here g and I refer to the gaseous and liquid states, respectively. Using data given in the table, please determine the values of AH and AG for this reaction for one mole of glucose, assuming that the reaction takes place at room temperature and atmospheric pressure. Substance CH 20. (glucose) 0 (9) H200...
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