When methanol, CH, OH, is burned in the presence of oxygen gas, O2, 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) + O,(g) → CO,(g) + 2 H,O(1) AH = –764 kJ %3D How much methanol, in grams, must be burned to produce 845 kJ of heat? mass:

When methanol, CH, OH, is burned in the presence of oxygen gas, O2, 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) + O,(g) → CO,(g) + 2 H,O(1) AH = –764 kJ %3D How much methanol, in grams, must be burned to produce 845 kJ of heat? mass:

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

3
A chemist measures the enthalpy change AH during the following reaction: COC1₂(9) + 4 NH3(9)→ CO(NH₂),(s) + 2NH4Cl(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. esc COC₁₂ (8) + 2NH₂(g) → CO(NH₂), (s) + NH₂Cl(s) 1 1 ẩCO(NH,),() + ≈NH,C() → † COCI,(8) + NH, (8) CO(NH₂)₂ (s) + 2NH₂Cl(s) → COCL, (g) + 4NH, (g) Explanation THE Check reaction I > AH=-559. kJ Costa ΔΗ kJ ☐ kJ KJ MacBook Pro x10 X S © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc You MOSISO L
The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is J/g-K.
Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol
When 29.5 mL of 0.500 M H2SO4 is added to 29.5 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g · ° C.)
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10
A 0.770-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0 °C. The reaction is 2 Li(s) + 2 H₂O(1)→ 2 LiOH(aq) + H₂(g) AHrxn=-446 kJ/mol Assuming no heat is lost to the surroundings, and that the final mixture has a specific heat capacity of 4.18 J/g °C, calculate the final temperature in °C. The enthalpy of fusion for ice is 6.02 kJ/mol.
M
Consider the combustion of propane: C3H (9) + 50, (9)→ 3CO, (9) + 4H2 O(1) AH = -2221 kJ A balloon is being inflated to its full extent by heating the air inside it. In the final stages of this process, the volume of the balloon changes from 4.00 x 10° L to 4.50 x 10° L by the addition of 1.4 x 10 J energy as heat. Assume that all the heat comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 50.% efficient? Mass =