Q 2 please 1) Calculate the standard enthalpy of reaction for the combustion of methane: loCO₂(g) + 2H₂O(g) →CH₂(g) +20₂(g), AH =?or 80-10Given that: AH, (CH₂(g))= -75 KJ/mol, AH', (CO₂(g))= -394 KJ/mol, and AH, (H₂O(g))= -284 KJ/mola) AH = -887 KJ/mol b) AH = +887 KJ/mol c) AH = -443.5 KJ/mol d) AH = 443.5 KJ/molrzFAN2) In the following figure, if AH₁ = 1000 KJ, AH3 = +1000 KJ, AH4 =-1000 KJ, calculate AH₂?a) AH-1000 KJ zorlub) AH 1000 KJc) AH₂= -3000 KJd) AH₂=3000 KJ3) A 300-g piece of iron at 70 °C is dropped into 266.4 mL of water at 24.0 °C. The final temperature of the waterand iron was measured as 40 °C. Calculate the specific heat of the iron. Assume the specific heat of the wateris 4.18 J/(g.°C)?a) S.Hiron = 2.97 J/(g.°C) b) S.Hiron = 2.55 J/(g.°C)c) S.Hiron 2.23 J/(g.°C) d) S.Hiron = 1.98 J/g °C)is zero (q=0)?c) Isobaric process4) In which process, heat absorbed or released by a systema) Adiabatic processb) Isothermal process5) Enthalpies of two reaction are given below;A+B →C+2D, AH,= - KJ/molC+E →A+F, AH₂=+x KJ/molCalculate AH for the reaction: 3A +2B+F→→3C+4D+Eb) AH=2x + ya) AH=2% - Yc) AH=X+YO Indicate which one of the following reactions result in a negative ASsys?a) H₂O(g) H₂O(s)c) CuSO4.(H₂O)s (s)CuSO4(s) + 5H₂O(g) (According to 2nd law of thermodynamics, in a spontaneousa) the entropy of the systemc) the energy of the universeDA- ΔΗ,AH, BAH, CAH₂b) CaCO3(s)d) CO₂(aq) + CO₂(g)d) Isochoric processCaO(s) + CO₂(g)A reaction is at equilibrium at a given temperature and constant pressure whena) AGsys > 0b) AGsys <0c) AGsys=0d) AH = -x - 2yprocess, which of the following always increasesb) the enthalpy of the systemd) the entropy of the universed) AHsys >0The enthalpy and entropy of vaporization of ethanol are 38.6 kJ/mol and 109.8 J/mol K, respectively. Whais the boiling point of ethanol, in °C? No 1 batza) 352 °CRETO.0b) 78.5 °C 1 c) 2.84 °Cd) 624 °C

NOTE : I HAVE BEEN ASKED TO SOLVE QUESTION NUMBER 2 ONLY , SO I AM GOING TO SOLVE ONLY THIS IF YOU…

2) In the following figure, if ΔΗ, = 1000 KJ, ΔΗ; = +1000 KJ, ΔΗ4 = -1000 KJ, calculate ΔΗ2? a) ΔΗz= -1000 KJ Α· ΔΗ, ΔΗ, ΒΔΗ, C-TH 3) A 300-g piece of iron at 70 °C is dropped into 266.4 mL of water at 24.0 °C. The final temperature of the water b) ΔΗz 1000 KJ c) ΔΗz= -3000 KJ d) ΔΗz= 3000 KJ D

2) In the following figure, if ΔΗ, = 1000 KJ, ΔΗ; = +1000 KJ, ΔΗ4 = -1000 KJ, calculate ΔΗ2? a) ΔΗz= -1000 KJ Α· ΔΗ, ΔΗ, ΒΔΗ, C-TH 3) A 300-g piece of iron at 70 °C is dropped into 266.4 mL of water at 24.0 °C. The final temperature of the water b) ΔΗz 1000 KJ c) ΔΗz= -3000 KJ d) ΔΗz= 3000 KJ D

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...

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