Question 2Thermochemistry2.1 Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent inmethanol can be utilized in a multitude of reactions. Consider the following reaction for thedecomposition of methanol:CH3OH(f) → CH,(g)+ /½02(g)Use Hess' Law to calculate the enthalpy change (in kJ-mol-') of this reaction, given the following knownthermochemical data:02(g) + 2H2(g) → 2H20(£)CH,(g) + H20(g)→ 3H2(g) + CO(g)H20(g) → H20(e)2H2(g) + CO(g) → CH3OH(f)AH, = -571.6 k] •mol-1AH, = 206.1 k] • mol-1AH, = -44.00 k] • mol-1AH,= -128.3 k] • mol-1 2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g of methanolwas placed in a bomb calorimeter (with a known heat capacity of 2.53 kJ-K'), together with 3.25 kg waterwith an initial temperature of 65.0 °C. After methanol is combusted, what will the temperature of the waterbe, given that the standard enthalpy of combustion of methanol is AH=-715.0 kJ-mol-1?

2.1) According to Hess Law of constant heat summation,"enthalpy change will be same whether the…

Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in methanol can be utilized in a multitude of reactions. Consider the following reaction for the decomposition of methanol: 2.1 CH3OH(e) → CH4(g) + 1½02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol') of this reaction, given the following known thermochemical data: 02(g) + 2H2(g) → 2H20(£) CH,(g) + H20(g) → 3H2(g) + CO(g) H20(g) → H20(e) 2H2(g) + CO(g) → CH3OH(?) AH, = -571.6 k] • mol- AH, = 206.1 k] · mol-1 AH, = -44.00 k] • mol-1 AH, = -128.3 k] • mol-1 %3!

Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in methanol can be utilized in a multitude of reactions. Consider the following reaction for the decomposition of methanol: 2.1 CH3OH(e) → CH4(g) + 1½02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol') of this reaction, given the following known thermochemical data: 02(g) + 2H2(g) → 2H20(£) CH,(g) + H20(g) → 3H2(g) + CO(g) H20(g) → H20(e) 2H2(g) + CO(g) → CH3OH(?) AH, = -571.6 k] • mol- AH, = 206.1 k] · mol-1 AH, = -44.00 k] • mol-1 AH, = -128.3 k] • mol-1 %3!

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

1
2.
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?
Test for SO, ion Take for instance you have a test solution and you will add 6 M HNO, drop by drop until it becomes acidic. Then you will add 0.1 M BaCl2 solution. What do you think will be formed?
When HCI(g) reacts with O₂(g) according to the following reaction, 28.6 kJ of energy are evolved for each mole of HCI(g) that reacts. Complete the following thermochemical equation. 4HCI(g) + O₂(g)2H₂O(g) + 2Cl₂(g) ΔΗ = 28.6| kj
Combustion of a hydrocarbon, X, is given by the equation: 2 X + 5 O2 (g) --> 4 CO2 (g) + 6 H2O (g) ∆H = -75.0 kJ Determine the standard enthalpy of formation of the hydrocarbon, X.
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.
A student has calibrated his/her calorimeter and finds the heat capacity to be 14.8 J/°C. S/he then determines the molar heat capacity of aluminum. The data are: 25.7 g Al at 100.0°C are put into the calorimeter, which contains 99.8 g H20 at 18.5°C. The final temperature comes to 22.6°C. Calculate the heat capacity of Al in J/mol-°C
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.
Use standard enthalpies of formation to determine ΔHorxnfor: 2Al(s) + 3Cl2(g) → 2AlCl3(s) Enter in kJ. Find the Internal energy for this reaction. Enter in kJ
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C
A bomb calorimeter has a heat capacity of 6.067 kJ/°C. A sample of vitamin (C31H4602) has an internal energy (DE) = -2.278 X 104 kJ/mol. When 1.434 g of the vitamin sample are burned in oxygen in the calorimeter, determine the final temperature in °C if the initial temperature is 14.51 °C.