Practice ProblemATTEMPT
Calculate the standard free-energy changes for the following reactions at
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Chemistry
- What 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_forwardH₂O(1) what is the enthalpy, AH, for this reaction? > AH = OO - ->> HCl(g) Resources HUAWEI P30 LEICA TRIPLE CAMERA XO₂ (s) AH4 = -668.7 kJ AHS = -44.0 kJ XC14(s) + 2 H₂O(1) - XO₂ (s) + 4 HCl(g) - AH3= -92.3 kJ a Hint Check Answer 10:32 AM 11/28/2022arrow_forwardGiven the following information: Bond C-H C-S S-H S=S Bond energy (kJ/mol) 414 259 347 452 Enthalpy of sublimation of CH3SH is 32.40 kJ/mol. (a) Estimate AH° in kJ for the formation of gaseous CH3SH in the following reaction: 2 CH4 (g) + S2 (g) ---> 2 CH3SH (g) Answer: kJ (b) Estimate AH° in kJ for the decomposition of solid CH3SH. 2 CH3SH (s) ---> 2 CH4 (g) + S2 (g) Answer: kJarrow_forward
- Given the following reactions and their enthalpies: ΔΗ (k/mol) H2(g) O2(g) 2H(g) 20(g) +436 +495 1 H>(g) + 02(g) → H;O(g) -242 (a) Devise a way to calculate AH for the reaction H,O(g) 2H(g) + O(g) (b) From this, estimate the H -0 bond energy.arrow_forwardDetermine Δ ngas for each of the following reactions: (a) MgCO3(s) → MgO(s) + CO2(g) mol (b) 2 H2(g) + O2(g) → 2 H2O(l) mol (c) HNO3(l) + ClF(g) → ClONO2(g) + HF(g) molarrow_forwardWhich has the smaller ΔHhydr in each pair of the Problem? Which ion has the lower ratio of charge to volume? Explain.(a) Br- or I- (b) Sc3+ or Ca2+ (c) Br- or K+(d) S2- or Cl- (e) Sc3+ or Al3+ (f) SO42- or ClO4-(g) Fe3+ or Fe2+ (h) Ca2+ or K+arrow_forward
- Use the data in Thermodynamic Properties to determine ΔH° for each of the following reactions.Please use the values in the Thermodynamic Properties to determine the expected number of significant figures. (a) Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) kJ(b) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) kJ(c) 2 Ag+(aq) + Pb(s) → 2 Ag(s) + Pb2+(aq) kJ(d) CH3COOH(l) + 2 O2(g) → 2 CO2(g) + 2 H2O(l) kJarrow_forwardCalculate So values for the following reactions by using tabulated So values from Appendix C.(a) 2 NOCl(g) Æ 2 NO(g) + Cl2(g)(b) Be(OH)2(s) BeO(s) + H2O(g)(c) HCl(g) + NaOH(aq) NaCl(s) + H2O(l)(d) 2 CH4(g) C2H6(g) + H2(g)arrow_forwardCalculate the standard molar enthalpy of formation of NO(g) from the following data: (A) N₂(g)+20,-2NO(g) (B) 2NO(g)+0,-2NO,(g) AH=66.4kJ AH° -114.1kJarrow_forward
- The following reactions can be used to prepare samples of metals. Determine the enthalpy change under standard state conditions for each.(a) 2Ag2 O(s) ⟶ 4Ag(s) + O2(g)(b) SnO(s) + CO(g) ⟶ Sn(s) + CO2(g)(c) Cr2 O3(s) + 3H2(g) ⟶ 2Cr(s) + 3H2 O(l)(d) 2Al(s) + Fe2 O3(s) ⟶ Al2 O3(s) + 2Fe(s)arrow_forwardUsing the following bond energies (in kJ/mol): BE(NºN) = 946; BE(Cl─Cl) = 243; BE(N─Cl) = 200 calculate the enthalpy change, DHrxn, for the following reaction in gaseous phase. N2(g) + 3Cl2(g) --> 2NCl3(g) (A) 475 kJ (B) 589 kJ (C) 1075 kJ (D) -1075 kJarrow_forwardUsing values from Appendix C of your textbook, calculate the value of AHO for each of the following reactions. (a) 2 C2Hg(g) + O2(g) = 2 C2H4(g) + 2 H2O(g) ΔΗ° - (b) CO(g) + H2O(g) = CO2(g) + H2(g) ΔΗ ΔΗ kJ (c) 6 C(graphite) + 6 H2O(I) = C6H1206(s) = kJ ΔΗ° = kJ (d) 2 HI(g) = H2(g) + I2(g) kJarrow_forward
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