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

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

Chapter1: Chemical Foundations

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

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6) What is the entropy change (J/K) for a system containing 3.00 mol of an ideal gas at 25.0 oC which is allowed to expand from 1.25 L to 5.00 L?
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
Consider the following reaction: C(graphite) + 1/2 O2 (g) → CO(g) Is it spontaneous under standard conditions at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS (universe). (Define reactants and products as the system.) S* (J/mol · K) A¡H° (kJ/mol) at 298 K (kJ/mol) Compound at 298 K C(s, graphite) 5.6 CO(g) 197.674 -110.525 CS2 (g) 237.8 116.7 CCL (e) 214.39 -128.4 Cl2 (g) 223.08 Si(s) 18.82 SİCL, (g) 330.86 -662.75 S(s, rhombic) 32.1 Br2 (e) 152.2 HBr(g) 198.70 -36.29 H2 (g) 130.7 H2O2 (e) 109.6 -187.78 O2 (g) 205.07 O yes O no
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
given rgetable of standard molar entropy values of each substance in the reaction below, what is the standard change in entropy, delta s, for the following reaction? 2CH3OH(g)+3OH2- 2CO2(g)+4H2O(g) Substance= CH3OH(g) S(J/mol•K) 240 Substance=O2(g) S(J/mol•K) 205 Substance=CO2(g) S(J/mol•K) 214 Substance=H2O(g) S(J/mol•k) 189 a. -352 J/K b. -1302 J/K c. 315 J/K d. 89 J/K E. 1830 J/K

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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