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Eliel et al. measured the value of delta rG degree = -6.02 kJ/mol at T =...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
Calculate the value of K, at 298 K, for each value of delta G degree. delta...
Calculate the value of K, at 298 K, for each value of delta G degree. delta G degree = 7.5 kJ/mol delta G degree = -9.0 kJ/mol
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol...
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.
DeltaH degree is +23 kJ mol^-1 of phosphine (PH_3) for the reaction Calculate Delta S degree...
DeltaH degree is +23 kJ mol^-1 of phosphine (PH_3) for the reaction Calculate Delta S degree for this reaction. Explain how this information allows you to determine the spontaneity or non-spontaneity of this reaction at any temperature. (S degree for PH_3 is 210 J K^-1 mol^-1.) Do these results indicate anything about the possibility of the existence of phosphine? Explain your answer.
Please show working! For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5)...
Please show working!
For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5) = -334.34 kJ/mol Delta G degree _f (SbCl_3) = -301.25 kJ/mol Delta H degree f (SbCl_5) = -394.34 kJ/mol Delta H degree _f (SbCl_3) = -313.80 kJ/mol Calculate the value of the equilibrium constant (K_P) for this reaction at 298 K.
need all of number 2 and three answered Calculate the missing value in each problem. Delta...
need all of number 2 and three answered
Calculate the missing value in each problem. Delta G = ?; AH = -217 kJ/mol; Delta S = 151 J/mol K; T = 451 K Delta G = 147 kJ/mol; Delta H = ?; Delta S = -98 J/mol K; T = 298 K Delta G = -20.4 kJ/mol; Delta H = 107 kJ/mol; Delta S = 211 J/mol K; T = ? How much heat is required to raise 37.3 g...
Calculate the standard entropy, Delta S_rxn^degree, of the following reaction at 25.0 degree C using the...
Calculate the standard entropy, Delta S_rxn^degree, of the following reaction at 25.0 degree C using the data in this table. The standard enthalpy of the reaction, Delta H_rxn^degree, is -633.1 kJ middot mol^-1. 3C_2 H_2(t) rightarrow C_6 H_6 (l) Delta S_rxn^degree = Number J middot K^-1 middot mol^-1 Then, calculate the standard Gibbs free energy of the reaction, Delta G_rxn^degree. Delta G_rxn^degree = Number kJ middot mol^-1 Finally, determine which direction the reaction is spontaneous as written at 25.0 degree...
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium...
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium mixture at 1000 K and 1767 torr are X_SO_2 = 0.310, X_O2= 0.190, and X_SO3= 0.500. Find K degree p and Delta G degree at 1000 K; assuming ideal gases, Find K_P at 1000 K. Find K degree C at 1000 K. K degree_P, and K degree_C have no units. Please enter them in 3 significant figures, e g. if the answer is 2.1,...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
T(N)=436 T= 436 c Question 1 The following gas phase reaction produces ethanol (C2H5OH) by catalytic...
T(N)=436
T=
436 c
Question 1 The following gas phase reaction produces ethanol (C2H5OH) by catalytic hydrogenation of acetaldehyde (CH3CHO). The reaction reaches equilibrium at a temperature of T= T(N) and a pressure of 3 bar: CH,CHO (g)+ H2 (g)C,H,OH (g) The reactive system initially contains 1.5 moles of Hydrogen (H2) for each mole of acetaldehyde (CH3CHO). The mixture is assumed to be an ideal gas. T(N) is the temperature corresponding to the student number as shown in the attached...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
Calculate the value of K, at 298 K, for each value of delta G degree. delta G degree = 7.5 kJ/mol delta G degree = -9.0 kJ/mol
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.
DeltaH degree is +23 kJ mol^-1 of phosphine (PH_3) for the reaction Calculate Delta S degree for this reaction. Explain how this information allows you to determine the spontaneity or non-spontaneity of this reaction at any temperature. (S degree for PH_3 is 210 J K^-1 mol^-1.) Do these results indicate anything about the possibility of the existence of phosphine? Explain your answer.
Please show working!
For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5) = -334.34 kJ/mol Delta G degree _f (SbCl_3) = -301.25 kJ/mol Delta H degree f (SbCl_5) = -394.34 kJ/mol Delta H degree _f (SbCl_3) = -313.80 kJ/mol Calculate the value of the equilibrium constant (K_P) for this reaction at 298 K.
need all of number 2 and three answered
Calculate the missing value in each problem. Delta G = ?; AH = -217 kJ/mol; Delta S = 151 J/mol K; T = 451 K Delta G = 147 kJ/mol; Delta H = ?; Delta S = -98 J/mol K; T = 298 K Delta G = -20.4 kJ/mol; Delta H = 107 kJ/mol; Delta S = 211 J/mol K; T = ? How much heat is required to raise 37.3 g...
Calculate the standard entropy, Delta S_rxn^degree, of the following reaction at 25.0 degree C using the data in this table. The standard enthalpy of the reaction, Delta H_rxn^degree, is -633.1 kJ middot mol^-1. 3C_2 H_2(t) rightarrow C_6 H_6 (l) Delta S_rxn^degree = Number J middot K^-1 middot mol^-1 Then, calculate the standard Gibbs free energy of the reaction, Delta G_rxn^degree. Delta G_rxn^degree = Number kJ middot mol^-1 Finally, determine which direction the reaction is spontaneous as written at 25.0 degree...
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium mixture at 1000 K and 1767 torr are X_SO_2 = 0.310, X_O2= 0.190, and X_SO3= 0.500. Find K degree p and Delta G degree at 1000 K; assuming ideal gases, Find K_P at 1000 K. Find K degree C at 1000 K. K degree_P, and K degree_C have no units. Please enter them in 3 significant figures, e g. if the answer is 2.1,...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
T(N)=436
T=
436 c
Question 1 The following gas phase reaction produces ethanol (C2H5OH) by catalytic hydrogenation of acetaldehyde (CH3CHO). The reaction reaches equilibrium at a temperature of T= T(N) and a pressure of 3 bar: CH,CHO (g)+ H2 (g)C,H,OH (g) The reactive system initially contains 1.5 moles of Hydrogen (H2) for each mole of acetaldehyde (CH3CHO). The mixture is assumed to be an ideal gas. T(N) is the temperature corresponding to the student number as shown in the attached...
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