What is the total change in entropy of the surroundings when10.0 g of ice melts at 25.0°C?AH fus6.01 kJ/molAS surr = -asys/Ta) 18.4 J/Kb) -18.4 J/Kc) 133 J/Kd) -11.2 J/Ke) 11.2 J/KH₂O(s)H₂O()Increasingentropy

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Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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At what temperature will the following reaction become spontaneous?3CO2(g) + 3H2O(l) ® CH3COCH3(g) + 4O2(g) DH = 854.00 kJ/mol and DS = 236.00 J/mol*K 3128. �C 3619. �C 1090. �C 3345. �C
Which one has a large entropy? 0.0200 moles of NaBr dissolved in 2.00 L of water or 0.0200 moles of CaCl 2 dissolved in 2.00 L of water. Explain
2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7
What is the entropy change, in J mol-1 K-1, when 100.0 g of water boils at 100.0 oC? (ΔHvaporization = 40.7 kJ/mol) Type in your answer as a whole number with no units.
1. Consider the following combustion reaction: C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) ∆Hrxn = -2044 kJ (a) Determine the sign of the entropy change for the above reaction. (b) Calculate the entropy change for the above reaction at 25°C. Does this match your predicted sign from (a)?
Calculate entropy change of a sample of 20 g of ice when it melts at 0oC under pressure of 1 atm. (fus H (H2O) = 6.0 kJ mol-1)
1)spontaneous or non spontaneous 2) the change in Gibbs free energy is negative or the change in Gibbs free energy is positive 3)positive or negative
8) a) Calculate AS°en for the following reaction given their respective standard molar entropy values. С-H- (6) + н, (в) сH. (8) S°(C,H2) = 200.9 J/mol K S°(H2) = 103.7 J/mol K S°(C;H4) = 219.3 J/mol K b) the reaction in 'part a' is endothermic, when would it be spontaneous?
Calculate the entropy change of 63.4 g of water that freezes into ice at 273.15 K. AHfus for water is 6.01 kJ/mol. J/K
32. The enthalpy and entropy of vaporization of ethanol are 38.6 kJ/mol and 109.8 J/mol · K, respectively. What is the boiling point of ethanol, in °C?a. 352°Cb. 78.5°Cc. 2.84°Cd. 624°Ce. Not enough information is given to answer the question
Give answer second question with explanation

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What is the total change in entropy of the surroundings when 10.0 g of ice melts at 25.0°C? AH fus 6.01 kJ/mol AS surr = -asys/T a) 18.4 J/K b) -18.4 J/K c) 133 J/K d) -11.2 J/K e) 11.2 J/K H₂O(s) H₂O() Increasing entropy