Practice ProblemBUILD
Given that the reaction
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Chemistry
- For which of the following is the change in entropy positive? Check all that apply. Explain. A. C 6 H 12 (l) C 6 H 12 (g)B. Dilution of 1.0 mL of 1.0 M NaOH with 90 mL of waterC. . 2 O 2 (g) + 2 SO (g) 2 SO 3 (g)D. grinding a large crystal of NaCl to powderE. Cooling water from room temperature to 15°C.arrow_forwardWhich of the following processes are endothermic? Check all that apply. H2O(l) ⟶⟶ H2O(s) H2O(g) ⟶⟶ H2O(l) 2 C8H18(l) + 25 O2(g) ⟶⟶ 16 CO2(g) + 18 H2O(l) CO2(s) ⟶⟶ CO2(g) 2 H2(g) + O2(g) ⟶⟶ 2 H2O(g) Δ?=−241.83??ΔH=−241.83kJ 2 Al(s) + 1.5 O2 ⟶⟶ Al2O3 Δ?=−1675.7??ΔH=−1675.7kJ Br2(g) ⟶⟶ 2Br(g) 1/2 N2(g) + O2(g) ⟶⟶ NO2(g) Δ?=33.1??ΔH=33.1kJarrow_forwardIf you have an enthalpy change of -102.2 kJ mol-1 at a temperature of 200C, determine the change in entropy assuming that the change is reversible and temperature remains constant. show process.arrow_forward
- Out atmosphere is composed primarily of nitrogen and oxygen, which coexist at 25°C without reacting to any significant extent. However, the two gases can react to form nitrogen monoxide according to the following reaction: N2(g) + O2(g) ⇌ 2NO(g) Calculate delta G° at 1940K. (Express answer using four significant figures.) Does the reaction become spontaneous with increasing temperature?arrow_forwardCalculate the temperature at which the following reaction becomes spontaneous. Compound ΔHof (kJmol)ΔHfo (kJmol) ΔSo (JK ⋅ mol)ΔSo (JK ⋅ mol) Cl2(g) 0.0 +223.1 ClNO2(g) +12.6 +272.2 NO(g) +91.3 +210.8 NO2(g) +33.2 +240.1 NOCl(g) +51.7 +261.7 PCl3(g) −287.2 +311.8 PCl5(g) −374.9 +364.6 PCl5(g) ↔ PCl3(g) + Cl2(g) (Answer with K unit )arrow_forwardH3. Consider a reaction for which the value of ΔG∘ = -9.199 kJ/mol at a 298.15 K. What is the value of Keq for this reaction at this temperature? Please give typed answerarrow_forward
- For a reaction with ΔH = 5.2767 kJ/mol and ΔS = 18 J/K•mol, at 20°C, the reaction is: Spontaneous Not Spontaneous At equilibrium. Please type answer note write by hend.arrow_forwardThe Gibbs free energy change (∆Go) of reaction A is 300 kJ/mol and that of reaction B is -400 kJ/mol. Which reaction is faster (A, B or impossible to determine with the given information)? Please explain answerarrow_forwardCompute ΔGo at 200.0 oC for each of the following reactions, which are important in the chemistry of coal. Assume that coal has the same thermodynamic properties as graphite. Substance ΔHo(kJ/mol) So(J/(mol*K)) C(graphite) 0 5.7 H2O(g) -241.83 188.835 CO(g) -110.5 197.7 H2(g) 0 130.680 O2(g) 0 205.152 CO2(g) -393.5 213.8 C(s, coal) + H2O(g) CO(g) + H2(g) C(s, coal) + O2(g) CO2(g) C(s, coal) + 1/2O2(g) CO(g) CO(g) + H2O(g) CO2(g) + H2(g)arrow_forward
- PCl3 + 3 CH3CH2OH --> 3 CH3CH2Cl + H3PO3 Compound ΔGof, kJ/mol Sfo, J/mol-K PCl3 -286 312 CH3CH2OH -175 161 CH3CH2Cl -53 190 H3PO3 -232 82 A. Find ΔGorxn. B. Is the reaction spontaneous at 25oC? C. Find ΔSorxn. D. Find ΔHorxn.arrow_forwardIn freezing a mole of liquid water at the freezing point, the enthalpy of fusion is 6.01 KiloJoules per mole. Answer the questions that follow. (A). What is the entropy change of this process (in Joules per Kelvin)? (B). What is the entropy change of the surroundings for this process (in Joules per Kelvin)? Express answer in THREE SIGNIFICANT FIGURES. (C). What is the total entropy change (or the entropy change of the universe) for this process (in Joules per Kelvin)? Express answer in THREE SIGNIFICANT FIGURES.arrow_forwardCalculate ΔGrxn at 308 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atm Group of answer choices +30.0 kJ +31.1 kJ +24.9 kJ -24.9 kJ -31.1 kJarrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning