Calculate AE when 162 g of C, H, undergoes combustion at 450. K and constant pressure.C₂H₂ (s) + 120, (g) 10CO₂ (g) + 4H₂O(g)AH = -5157 kJUse 128.18 g/mol as the molar mass of C₁H₂.Use 5 sig figskJ2 AttemptsSubmit

Answered: Image /qna-images/answer/bc996737-3d87-4dd5-9690-2cdbb4522d96.jpg

Calculate AE when 162 g of CH undergoes combustion at 450. K and constant pressure. 10CO₂ (g) + 4H₂O (g) C₁H (s) + 120₂ (9) AH = -5157 kJ Use 128.18 g/mol as the molar mass of C₁H₂. Use 5 sig figs kJ 2 Attempts Submit

Calculate AE when 162 g of CH undergoes combustion at 450. K and constant pressure. 10CO₂ (g) + 4H₂O (g) C₁H (s) + 120₂ (9) AH = -5157 kJ Use 128.18 g/mol as the molar mass of C₁H₂. Use 5 sig figs kJ 2 Attempts Submit

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

(a) John performed a bomb calorimetry experiment using 2.147 g of CSH10O5. The temperature of the calorimeter rose from 24.18°C to 28.33°C. Given the heat capacity of the calorimeter and contents was 4.567 kJ/°C, determine the heat of combustion of C3H10O5 in kilojoule per mole.
Using the provided table, determine the enthalpy for the reaction C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AH¡ (kJ/mol) C3H® (g) -108.4 O2 (g) CO2 (g) -393.5 H2O (g) -241.8
2. Consider the following thermochemical equations: C(graphite) + O2 (g) → co2 (g) AH°rn = -393.5 kJ H2 (g) + % 02 (g) → H;0 (/) AHO = -285.8 kJ 2 C:Hs (g) + 702 (g) → 4 CO2 (g) + 6 H20 (1) AH°rn = -3119.6 kJ a. Derive the thermochemical equation describing the combustion of two moles of C(graphite). b. Derive the thermochemical equation describing the combustion of three moles of H2 (g). c. Derive the thermochemical equation describing the synthesis of one mole of C,Hg (9) from carbon dioxide and water. d. Use Hess's Law and the three thermochemical equations you derived in parts a-c to determine the AH°ran for the following reaction: 2C (graphite) + 3 H2 (g) → C;Hs (g)
To study the possible amount of energy generated by a person, the person can be roughly viewed as a constant pressure calorimeter using table sugar (sucrose, C12H22O11) as the energy generator. The reaction of table sugar in a calorimeter is given by: C12H22O11(s) + 12O2(g) ----------> 12CO2(g) + 11H2O(g) a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. Calculate the enthalpy of combustion per mole of sugar utilization. c. Does the result of your calculation make sense?
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
(c) Consider the following chemical reaction: C;Hs(g) + H2(g) C2H6(g) + CH4(g) ΔΗ? %3D Calculate the enthalpy change for the reaction above using Hess's law. Thermochemical dat: H:(g) + ½O2(g) H2O(1) AH° =-285.8 kJ AH°combustion for CH4(g) AH° =-890.0 kJ/mol %3D CO:(g) C(s. graphite) + O:(g) AH° = +393.5 kJ AH°combustion for C2H6(g) AH = -1560.0 kJ/mol AH°, for C3H$(g) AH° =-103.8 kJ/mol
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 8.000 g tablet of benzoic acid (C6H₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 10.00 °C to 47.00 °C over a time of 5.8 minutes. olo Next, 5.940 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 10.00 °C to 55.55 °C. Ar chemical reaction Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: "bomb" A "bomb" calorimeter. C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) 4 Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
The combustion of neopentane is described by the reaction: C5H12(s) + O2(g) → CO2(g) + H2O (unbalanced) AH = -3456 kJ/mol neopentane %3D If 100.0 milligrams of neopentane is burned in a bomb calorimeter to heat 100.0 mL of water at 25°C, what would be the final temperature of water in °C? The specific heat of water is 4.184 J/g°C, The MW of neopentane is 72.15 g/mol. Answer in four significant figures. Indicate the unit.
7.Using the following standard enthalpies of reaction4NH3(g) + 7 O2(g) 4 NO2(g) + 6 H2O(l)H ̊rxn= -1395 kJN2(g) + 2 O22 NO2(g)H ̊rxn= +67.4 kJFind the standard enthalpy of reaction for the equation:2N2(g) + 6 H2O(l) 4 NH3(g) + 3 O2(g) Based on your work above, determine the standard enthalpy of reaction for the following equation:N2(g) + 3 H2O(l) 2 NH3(g) + 3/2 O2(g)
The combustion of 1.925 g of propanol (C₂H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.14 K. The heat capacity of the bomb calorimeter is 15.61 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. kJ/mol ΔΗ = TOOLS x10
please I want an answer question
A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation:B2H6(g)+3O2(g)➔B2O3(s)+3H2O(g)ΔHcombustion for this process is –1958 kJ/mol. Assume that 0.411 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 22.61°C. What is the final temperature of the calorimeter? The answer is not 18.922°C