Answered: Using the provided table, determine the…

Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction C(s) + CO, (g)→ 2 CO (g) Substance AH¡ (kJ/mol) C (s) CO2 (g) -393.5

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

Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction 2 NH3(g) + 3 N₂O (g)→ 4 N₂ (g) + 3 H₂O (1) Substance NH3 (9) N₂O (g) N₂ (g) H₂O (1) AHf (kJ/mol) -46.2 81.6 0 -285.8
(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.
THERMODYNAMICS: A 1.09 g sample of acetic acid (HC2H2O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 KJ°C. contained 7g of water. The temperature of the calorimeter and its contents increased from 24.13°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 gimol. (Round off the final answer to ONE decimal place. Do not include the unit.)
Calculate the enthalpy of combustion (kJ/mol) of methyl linoleate (C₁₉H₃₄O₂), an important component of many biodiesel fuels made from corn oil and methanol, given the following standard enthalpies of formation: CO₂(g) = -393.5 kJ/mol H₂O(l) = -285.8 kJ/mol C₁₉H₃₄O₂(l) = -645.7 kJ/mol
When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
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
The heat capacity of a bomb calorimeter was determined by burning 6.85 g of methane (energy of combustion = -803 kJ/mol CH4) in the bomb. The temperature changed by 11.1°C. (a) What is the heat capacity of the bomb? kJ/°C (b) A 14.7-g sample of ethanol (C₂H5OH) produced a temperature increase of 12.8°C in the same calorimeter. What is the energy of combustion of ethanol (in kJ/mol)? kJ/mol
Find the enthapy change for the reaction below in kJ . 4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(g) ΔH= ? Given : (NH3(g)) = -46.1, (NO(g)) = + 90.3 kJ/mol and (H2O(g)) = -241.8 kJ/mol.
Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g) Substance ∆Hf° (kJ/mol) C₃H₈ (g) -108.4 O₂ (g) 0 CO₂ (g) -393.5 H₂O (g) -241.8
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (C6H-CO₂H) 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 14.00 °C to 33.17 °C over a time of 6.8 minutes. Next, 4.040 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 14.00 °C to 39.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ, per mole of…
Given the following two reactions:(1)Fe(s) + Cl2(g)->FeCl2(s) H(1) = -341.8 kJ(2)Hg(l) + Cl2(g)->HgCl2(s) H(2) = -224.3 kJcalculate the enthalpy change for the following reaction:(3) FeCl2(s) + Hg(l)-> Fe(s) + HgCl2(s) H(3) = kJ
A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.