Practice problemBUILD
For each reaction, determine the value of
(a)
(b)
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Chemistry
- (22) Using the provided tabulated values, calculate AS°ran for the following reaction that occurs at 25°C: CS2 (g) + 3 Cl2 (g) → CCL4 (g) + S;Cl2 (g) (A) (B) 168.1 J/K -278.2 J/K 278.2 J/K (C) (D) -168.1 J/K 391.2 J/K (E) ldarrow_forward#2 For each reaction, find the value of ΔSo. Report the value with the appropriate sign. (a) 3 NO2(g) + H2O(l) →2 HNO3(l) + NO(g) =____J/K (b) N2(g) + 3 F2(g) →2 NF3(g) =____J/K (c) C6H12O6(s) + 6 O2(g) →6 CO2(g) + 6 H2O(g) =____J/Karrow_forwardUse the data below to determine the ΔHrxn for the following reaction: S=S(g) + H2(g) è H-S-S-H(g) (S=S: 425 kj/mol; S-S: 286 kj/mol, H-S: 363 kj/mol, H-H: 432 kj/mol )arrow_forward
- ind ΔH for the reaction C3H8 (l) + 5O2(g) --> 3CO2(g) + 4H2O(l) ΔHrxn = ? Given: [CO2(g)] = -393.5 kJ/mol, [H2O(l)] = -285.8 kJ/mol, [C3H8(l)] = -103.8 kJ/mol) (Your answer is in kJ and has one digit after the decimal. Enter only the number) Careful with sign.arrow_forward1. (a) Based on the information below, determine ΔGrxn (in kJ) for the following reaction: 2A(g) + B(g) → 2C(g). A → B ΔGrxn = 75kJ ½ C → B ΔGrxn = 45kJ C → A ΔGrxn = -25kJ Answer ________________ 2. The reaction in the previous question is exothermic. Which of the following statements is true? A The reaction is spontaneous at all temperatures. B The reaction is spontaneous at high temperatures. C The reaction is spontaneous at low temperatures. D The reaction is not spontaneous at any temperature.arrow_forwardWhat is the ΔE for a system which has the following two steps:Step 1: The system absorbs 60 J of heat while 40 J of work are performed on it.Step 2: The system releases 30 J of heat while doing 70 J of work.(a) 0 J(b) 100 J(c) 30 J(d) 90 Jarrow_forward
- 4. Consider the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) having AH = -484 kJ/mol. Determine the magnitude of the heat exchanged with the surroundings when 3 mol of H2 and 3 mol of O2 react. (a) 161 kJ (b) 323 kJ (c) 484 kJ (d) 726 kJ (e) 1452 kJ (f) 2904 kJarrow_forwardWrite the balanced overall equation for the following process, calculate ΔHₒᵥₑᵣₐₗₗ, and match the number of eachequation with the letter of the appropriate arrow in Figure .a)P₄(s)++6Cl₂(g)→4PCl₃(g) ΔH=1148 kJ 4PCl₃(g)+4Cl₂(g)→4PCl₅(g) ΔH=460 kJ.Calculate ΔHₒᵥₑᵣₐₗₗarrow_forwardWith hypothetical equation Calculate the value of ΔH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g) 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l) ΔH = -1,058.1 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (l) ΔH = -1,594.2 kJarrow_forward
- Chemistry 5.2) Calculate AE for the combustion of hydrogen chloride at 25°C. (The ideal gas constant R= 8.314 J/K.mol) 4HC1 (g) + O2 (g) 2Cl₂ (g) + 2H₂O(g) A)-852.9 kJ B)-253.2 kJ C) -732.4 kJ D) -111.9 kJ E)-393.5 kJarrow_forwardUsing values from Appendix C of your textbook, calculate the value of Ho, So, and Go for each of the following reactions at standard temperature (298 K). Next calculate G if ALL of the GASSES in the reaction have partial pressures of 0.2 atm.(a) 3 NO(g) NO2(g) + N2O(g) Ho = kJ/mol So = J/mol-K Go = kJ/mol If all gasses have partial pressures of 0.2 atm then G = kJ/mol.arrow_forwardBe sure to answer all parts. For the gaseous reaction of carbon monoxide and chlorine to form phosgene (COC1₂), perform the following calculations. (a) Calculate the ASº at 298 K (AH = -220. kJ/mol and AG =-206 kJ/mol). kJ/mol·K (b) Assuming that AS and AH change little with temperature, calculate AG at 450. K. kJ/molarrow_forward
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