Suppose that methane, acetylene, and water vapor can be converted into propanol through the balanced chemical equation below:CH₂(g) + C₂H₂(g) + H₂O(g) →→→ C₂H₂O(1)The standard heats of formation for these compounds are:CH4 (g): 4H = -74.82 kJ/mol= 226.7 kJ/molC₂H₂(g): H0H₂O(g): AH= -241.8 kJ/molC3H8O (1): AH = -304.6 kJ/molDetermine the standard enthalpy change for the above reaction converting methane to propanol.kJ

Answered: Image /qna-images/answer/601705c1-2f4a-4312-9625-2e411a53b815.jpg

Suppose that methane, acetylene, and water vapor can be converted into propanol through the balanced chemical equation below: CH₂(g) + C₂H₂(g) + H₂O(g) → C₂H₂O(1) The standard heats of formation for these compounds are: CH4 (g): AH = -74.82 kJ/mol C₂H2 (8): AH = 226.7 kJ/mol H₂O(g): AH = -241.8 kJ/mol C3H8O (I): AH = -304.6 kJ/mol Determine the standard enthalpy change for the above reaction converting methane to propanol. kJ

Suppose that methane, acetylene, and water vapor can be converted into propanol through the balanced chemical equation below: CH₂(g) + C₂H₂(g) + H₂O(g) → C₂H₂O(1) The standard heats of formation for these compounds are: CH4 (g): AH = -74.82 kJ/mol C₂H2 (8): AH = 226.7 kJ/mol H₂O(g): AH = -241.8 kJ/mol C3H8O (I): AH = -304.6 kJ/mol Determine the standard enthalpy change for the above reaction converting methane to propanol. kJ

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

When 0.514 g of biphenyl, C12H10, undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 C to 29.4 C. Find ∆Urxn for the combustion of biphenyl. The bomb calorimeter contains 750.0 mL of water and has a heat capacity of 2.72 kJ/C.
A mass of 0.395 g of CHalg) is combusted in a bomb calorimeter that has a heat capacity of 785 C and contains 1.345 kg of water. If the temperature of the water in the calorimeter rises from 19.50°C to 28,50 C, what is energy of combustion of CH in k/mol? (Cwater4.184 J/gC) -289 k/mol 75.77x10klimol 544x10 kJ/mol 6-146klimol -234x 10 kmal
How much energy in kJ is released in burning 2.43 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol) The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ) ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8 Round your answer to 2 decimal places.
Consider the following balanced combustion reaction: C7H16(l) + 11 O2(g) → 7 CO2(g) + 8 H2O(g) ΔrH°= -1160 kJ/mol If the density of C7H16(l) is 0.68 g/mL, how much heat (in J and scientific notation) is released if 125 mL of C7H16(l) undergoes complete combustion?
Using the data given, calculate the standard enthalpy of combustion of C₂H₆ in kJ/mol? Thermochemical Data H₂(g) + 1/2O₂(g) → H₂O(l) ΔH°= –286 kJ C₂H₄(g) + H₂(g) → C₂H₅(g) ΔH°= –137 kJ C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(l) ΔH°= –1412 kJ A) –1275 kJ B) –1548 kJ C) –31561 kJ D) +1834 kJ
How much energy in kJ is released in burning 1.63 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol) The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ) ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8 Round your answer to 2 decimal places.
Consider the following reaction carried out under constant pressure 5Cl2(g) + 2P(s) → 2PCl5(g) Δ Hrxn = -749.8 kJCalculate the heat associated with the complete reaction of 84.0 g of Cl2 with 20.6 g of P. -6.15×102 kJ -1.78×102 kJ -4.99×102 kJ -8.88×102 kJ -2.50×102 kJ
When burning 0.25 g of CH3OH in a calorimeter bomb with a heat capacity of 1.50 kJ / 0C, it increases the temperature of the calorimeter bomb by 0.45 0C. How many kg of CH3OH (methyl alcohol) should be burned to obtain 2.76x105 kJ of heat? (CH3OH = 32 g / mol)
Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. Is the following statement true or false? This process is exothermic. True False
In the following reaction, what is the quantity of heat (in kJ) released when 4.93 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol
Acetylene burns in air according to the following equation. C2H2(g) + 5/2 O2(g) 2 CO2(g) + H2O(g) H0rxn = -1255.8 kJ Given that H0f of CO2(g) = -393.5 kJ/mol and H0f of H2O(g) = -241.8 kJ/mol, what is H0f of C2H2(g)?
How much heat is produced when 0.480 mol of methane is burned under standard conditions. Enthalpy of combustion of methane = -891 kJ/mol. - A) -891 kJ B 428 kJ -222 kJ -644 kJ -428 kJ