When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown inthe combustion reaction.CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(1) AH = -764 kJBased on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 gof oxygen?heat:Which reactant is limiting?methanoloxygenkJ

Answered: Image /qna-images/answer/a992fb76-c503-4571-993e-4c094fc92f4d.jpg

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown in he combustion reaction. CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(l) AH-764 kJ Based on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 g af oxygen? eat: Which reactant is limiting? methanol oxygen kJ

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown in he combustion reaction. CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(l) AH-764 kJ Based on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 g af oxygen? eat: Which reactant is limiting? methanol oxygen kJ

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

The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine molecule consumed [2 Na(s) + Cl2(g) → 2 NaCI(s)]. How much heat is released (in kJ) if 4.785 g of Na are consumed in the reaction?
The common fertilizer NH,N0;(s), can explosively decompose according to the following reaction. What is the heat released when 80.06 g of NH,NO;(s) explodes? Molar mass of NH,NO:(s)= 80.06 g/mol. 28. 2 NH,NO3(s) → 2 N2(g) + O2(g)+4 H,O (g) AH = -236.15 kJ -472.3 kJ A) B) -236.15 kJ -118.08 kJ D) -59.04 kJ
Acetylene, C,H2, is used in welding torches. It releases a lot of energy when burned in oxygen. The combustion of one gram of acetylene releases 48.2 kl_ A-0.750-gram sample of acetylene is burned in a bomb calorimeter (heat capacity = 1.117kJ/°C) that contains 800.0 g of water. The final temperature of the bomb and water after combustion is 35.2°C. What is the initial temperature of the bomb and water?
In the following reaction, how much heat is generated when 3.21 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
In a popular television series, the two characters use thermite to assist with breaking into a chemical storage facility because the reaction between aluminum and iron(III) oxide produces a tremendous amount of heat. If they began with 10.0 g of Al, how many kJ of heat would be released? 29. 2 Al(s) + Fe,O3(s) → Al,O;(s) + 2 Fe(s) AH = -852 kJ 158 kJ A) B) 236 kJ 472 kJ D) None of the above
Kindly complete the following questions (showing all your work).
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g) → 10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g) → AsBr3(g) ΔH = -336.4 kJ/mol As4(s) + 5 O2(g) → As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g) → AsBr5(g) ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g) → Br3AsO(g) ΔH = -295.7 kJ/mol
75.0 mL of 1.80 M CuSO 4 solution is mixed with 150 mL of 1.80 M NAOH solution in a coffee cup calorimeter of negligible heat capacity. If the initial temperature of the two solutions are both 21.0 degrees C, and the final temperature of the mixed solution is 27.1, how much heat was released by the reaction? Assume density of solution d is 1.00 g/mL and that the solution has the same specific heat as water. The thermochemical equation is: CuSO4 (ag) + 2NAOH (ag) --> Cu(OH)2 (s) + Na SO4 (ag) AH xn = - 42.3 kJ/mol rxn Hint: no limiting reagent, substances are presented in correct molar ratios. O 6180 J O 9270 J O 3120 J O 5740 J O 9300 J O 1250 J O 6230 J O 3380 J
4. 30.0 g of a substance (molar mass: 46 g/mo) required 262 J of heat to raise its temperature from 32.0°C to 37.4°C. What is the specific heat per gram and per mole of this substance?
When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ