Predict the signs of delta H (Enthalpy) and delta S (Entropy) for the evaporation of water at 85 C
What is delta S? Predict the signs of Delta S and Delta H for the freezing of water into ice at 273 K. a. Delta H > 0 and Delta S < 0 b. delta H = 0 and Delta S > 0 c. Delta H < 0 and Delta S < 0 d. Delta H > 0 and Delta S = 0 e. Delta H < 0 and Delta S > 0
what are the signs of entropy change and enthalpy change for the combustion reaction of magnesium? Why? 2Mg(s) + O2(g) -> 2MgO(s) A) Delta H > 0, Delta S > 0 B) Delta H > 0, Delta S < 0 C) Delta H < 0, Delta S > 0 D) Delta H < 0, Delta S < 0
What is the meaning of delta H (change in enthalpy), delta S (change in entropy) and delta G (change in Gibbs free energy) as it relates to mixing two liquids together? In what situations is each of these variables negative/positive?
8. Part A. (9 pt) For the reaction below, predict the signs for delta H system, delta S system, and delta S surrounding, AND explain your answer for each. 8. Part A. (9 pt) For the reaction below, predict the signs for AHºsys, ASºsys, and AS surr, and EXPLAIN your answers.
What are the signs (+ or -) for delta H, delta S, and -T(delta S) which are required to produce the following signs (+ or -) of delta G. Think about the equation delta G = delta H - T(delta S). 1. If delta G is negative 2. If delta G is either positive or negative (there are 2 solutions) 3. If delta G is negative
We have an unknown liquid. For its evaporation, what are the signs (positive or negative) for its enthalpy change, its entropy change, and the change in the entropy of the surroundings/environment?
In terms of the algebraic signs of delta H and delta S, under which of the following circumstances will a change be spontaneous? a) at all temperatures? b) at low temperatures but not high temperatures? c) at high temperatures but not at low temperatures?
Predict the signs, comment and then calculate the enthalpy and entropy changes for the reaction of combustion ofmethane at 500 K. Will the reaction be spontaneous at 500 K? CH4(g) + 2 O2(g) → CO2(g) + 2H2O(g) We give: The enthalpies of formation of the products at 298.15 K in kJ/mol are: ∆Hf(CO2) = - 393.51; ∆Hf(H2O) = - 241.82; ∆Hf(CH4) = -74.81. The heat capacities at constant pressure in J.mol-1.K-1: Cp(CO2) = 37.11; Cp(H2O) = 33.58; Cp(CH4) = 35.31;...
Predict the sign of the entropy change, Delta S degree, for each of the reaction displayed. Drag the appropriate items to their respective bins. Calculate the standard entropy change for the reaction 2Na(s) + CI_2 (g) rightarrow 2NaCl(s) using the data from the following table: Express your answer to four significant figures and include the appropriate units.
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol