Need asap The standard enthalpy of combustion of propane, C3Hg, is -2.220 x 103 kJ mol-1 at 400 K. Use the data below, andKirchhoff's law, to calculate the standard enthalpy of combustion at 600 K. The reaction involved is:C3H8 (9) + 5 O2(g) → 3 CO2(g) + 4H₂O(g)Cp,m (J K-1 mol-1): C3H8 (g) = 73.6; O2(g) = 29.4; H₂O(g) =33.6; CO2(g) =37.1-3395 kJ mol-1- 2195 kJ mol-12595 kJ mol-1500 kJ mol-1 An important industrial chemical process is the production of nitric acid. One of the important step in the synthesis of nitricacid is the conversion of ammonía to nitric oxide:4NH3(g) + 502(g) →→ 4NO(g) + 6H₂O(g)Calculate Hºrxn for this reaction. Given the following data:Hᵒf [NH3(g)] = -45.9 kJ/mol;Hᵒf [NO(g)] = 90.3 kJ/mol;Hᵒf [H2O(g)] = -241.8 kJ/mol-105.6 kJO-906.0 kJ197.4 kJ-197.4 kJ

Given : ∆H° for combustion of methane at 400 K = -2.220 x 103 KJ/mol T1 = 400 K T2 = 600 K

The standard enthalpy of combustion of propane, C3Hg, is -2.220 x 103 kJ mol-1 at 400 K. Use the data below, and Kirchhoff's law, to calculate the standard enthalpy of combustion at 600 K. The reaction involved is: C3H8 (g) + 5 O2(g) → 3 CO2(g) + 4H₂O(g) Cp,m (J K-1 mol-1): C3H8 (g) = 73.6; O2(g) = 29.4; H₂O(g) =33.6; CO2(g) =37.1 -3395 kJ mol-1 - 2195 kJ mol-1 2595 kJ mol-1 500 kJ mol-1

The standard enthalpy of combustion of propane, C3Hg, is -2.220 x 103 kJ mol-1 at 400 K. Use the data below, and Kirchhoff's law, to calculate the standard enthalpy of combustion at 600 K. The reaction involved is: C3H8 (g) + 5 O2(g) → 3 CO2(g) + 4H₂O(g) Cp,m (J K-1 mol-1): C3H8 (g) = 73.6; O2(g) = 29.4; H₂O(g) =33.6; CO2(g) =37.1 -3395 kJ mol-1 - 2195 kJ mol-1 2595 kJ mol-1 500 kJ mol-1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 96QRT

See similar textbooks

Similar questions

Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
Benzoic acid of mass 1.40 g is reacted with oxygen in a constant volume calorimeter to form H2O(l) and CO2(g) at 298 K. The mass of the water in the inner bath is 1.40×103g. The temperature of the calorimeter and its contents rises 2.84 K as a result of this reaction. Part A Calculate the calorimeter constant. The standard enthalpy of combustion of benzoic acid at 298 K is −3227 kJ⋅mol−1. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1.
A sample of the sugar d-ribose (C5H10O5) of mass 0.727 g was placed in a calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for which the internal energy of combustion is −3251 kJ mol−1, gave a temperature rise of 1.940 K. Calculate the enthalpy of formation of d-ribose.
What is the standard enthalpy of isomerization (kJ/mol) of propanol to isopropanol in the liquid state?
Estimate the enthalpy of vaporization of water at 100 °c from its value at 25 °c, 44.01 kJ mol-1, given the constant pressure molar heat capacities of 75.29 J K-1 mol-1 and 33.58 J K-1 mol-1 for liquid and gas, respectively.
The hydrocarbons acetylene (C2H2) and benzene (C6H6)have the same empirical formula. Benzene is an “aromatic”hydrocarbon, one that is unusually stable because of its structure.(a) By using data in Appendix C, determine the standardenthalpy change for the reaction 3 C2H2(g)-----> C6H6(l).(b) Which has greater enthalpy, 3 mol of acetylene gas or1 mol of liquid benzene? (c) Determine the fuel value, inkJ/g, for acetylene and benzene.
The complete combustion of solid fumaric acid, HOOCCH=CHCOOH, in a bomb calorimeter released 1333 kJ mol -1 of heat at 298 K. Calculate (a) the internal energy of combustion, (b) the enthalpy of combustion . (c) Usetabulated values for the standard enthalpy of formation of water and carbon dioxide to calculate the enthalpy of formation of solid fumaric acid.
A) For nitrogen gas the values of Cv and Cp at 25°C are 20.8 J K−1 mol−1 and 29.1 J K−1 mol−1, respectively. When a sample of nitrogen is heated at constant pressure, what fraction of the energy is used to increase the internal energy of the gas? B) How much energy (in KJ) is required to raise the temperature of 136.4 g N2 from 25.0°C to 87.0°C in a vessel having a constant volume?