Use the References to access important values if needed for this question. Consider the reaction: NH4Cl(aq)-NH3(g) + HCl(aq) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.25 moles of NH4Cl(aq) react at standard conditions. AS system J/K Submit Answer Retry Entire Group 8 more group attempts remaining

Use the References to access important values if needed for this question. Consider the reaction: NH4Cl(aq)-NH3(g) + HCl(aq) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.25 moles of NH4Cl(aq) react at standard conditions. AS system J/K Submit Answer Retry Entire Group 8 more group attempts remaining

Chemistry

10th Edition

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

Section: Chapter Questions

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

See similar textbooks

Similar questions

A 1 mol quantity of hydrogen gas sample was heated at constant pressure from a temperature of 300 K to 500 K. With the entropy transformation process as a function of temperature variation, the heat capacity equation at constant pressure was estimated , Cp = 6.9469 - 0.199 x 10-3 T + 4.808 x 10-7 T2 (J K-1mol-1). Determine the entropy change of the process.
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40g of ethylbenzene (PhEt) and 50g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead, you mix 40g of benzyl alcohol (PhMeOH) into 50g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as: ΔΔG = ΔmixG [PhMeOH ∶ PhH] − ΔmixG [PhEt ∶ PhH] What do you expect the sign of ΔΔG to be? (ΔΔG<0, ΔΔG≈0, or ΔΔG>0)Briefly justify your answer.
Solid iodine, I2(s), has an enthalpy of sublimation ΔHsubl = 62.4 kJ mol-1. Suppose 5.36 g of iodine at a constant temperature of 35.0 oC is allowed to sublime into the atmosphere at a temperature of 50.8 oC. 1.Calculate the entropy change of the system (i.e. the iodine) in J K-1. Enter your answer into the first answer field in accordance with the question statement
Consider the reaction:2C2H6(g) + 7O2(g)4CO2(g) ---------> 6H2O(g)Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.69 moles of C2H6(g) react at standard conditions. S°system = _______ J/K
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50 g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40 g of ethylbenzene (PhEt) and 50 g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead you mix 40 g of benzyl alcohol (PhMeOH) into 50 g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as:ΔΔG = ΔmixG[ PhMeOH ∶ PhH ] − ΔmixG[ PhEt ∶ PhH ]What do you expect the sign of ΔΔG to be? ( ΔΔG < 0, ΔΔG ≈ 0, or ΔΔG > 0 )Briefly justify your answer.
Use the database on the textbook to calculate the entropy change of the following reaction under standard condition 1bar and 298 K: 2C2H6 (g) + 7O2 (g) = 4CO2 (g)+ 6H2O (L) ΔreactionS = _________ J/K/ (mol reaction). 4 sig. fig. per mole of reaction, not per mole of any subject. The data is copied from the appendix here material standard entropy ( J/K/mol) C2H6 229.60 O2 205.138 CO2 213.74 H2O(L) 69.91
Calculate the standard reaction entropy at 298 K of (a) 2 CH3CHO(g) + O2(g) → 2 CH3COOH(I)(b) 2 AgCI(s) + Br2(l) → 2 AgBr(s) + Cl2(g)(c) Hg(l) + Cl2(g) → HgCI2(s)(d) Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)(e) C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(l)
Part b-- Standard entropy = 205 J/mol K
Consider the reaction:1. 2SO2(g) + O2(g)2SO3(g)Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.06 moles of SO2(g) react at standard conditions. S°system = J/K Submit Answer 2. Consider the reactionFe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.80 moles of Fe2O3(s) react at standard conditions. S°surroundings = J/K Submit Answer
Calculate the standard reacton entropy at 298K of the following: 1. CH3CHO (g) + O2 -----→ CH3COOH (l) 2. Sucrose [C12H22O11(s)] + O2(g) ----→ CO2 (g) + H2O (l) 3. Zn(s) + Cu2+ (aq) ---→ Zn2+ (aq) + Cu (s)
Calculate the standard entropy change for the following process at 298 K:H2(g)+F2(g)⟶2HF(g) The standard entropies are as follows: S∘H2(g)=130.7Jmol K, S∘F2(g)=202.8Jmol K, and S∘HF(g)=173.8Jmol K. Include a negative sign in your answer, if appropriate. Round your answer to the nearest tenth.
Calculate the standard entropy of reaction, ΔS° (in J K−1 mol−1), for: Na2CO3(aq) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g) given the following data: Na2CO3(aq) HCl(aq) NaCl(aq) H2O(l) CO2(g) S° (J K−1mol−1) 134.98 56.5 115.5 69.91 213.74 Here are the possible answers: +323.2 -207.7 +266.7 +207.7 -266.7