ICottizO,+60276CO2+ lott20+362,5 KJ7660ztottzO+362,5 KJFinnd he amount of hect releasedwhen 188.9 gram s of casbon dicxideIS produced when Glucose andWAADAh Oxygen react.of carbon dicxideSluCOse arLELESEMCE MO DISCO32ESAICEMDIEEGO

Answered: Image /qna-images/answer/e150f772-4d70-4a3c-9862-7c9c30f7d7c6.jpg

Answered: ICottizO, o +6027 LoCOz+ Lot2O+362,5 KJ…

ICottizO, o +6027 LoCOz+ Lot2O+362,5 KJ Find the amount of heat released when 18.9 grams of carbon dioxide 1S produced when Glucose and WAADAh oygen react.

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

Calculate the quantity of energy transferred (q), in kJ, by the combustion of 177 mL of acetone (C3H6O)? C3H6O(l) + 4 O2(g) → 3 CO2(l) + 3 H2O(g) ΔHrxn = -1790 kJ Given: The density of acetone is 0.788 g/mL and its molar mass is 58.08 g/mol IMPORTANT: Enter both the sign and the value (no units), using 3 significant figures.
When copper(II) sulfate pentahydrate (CuSO4'5 H₂O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is: heat CuSO4-5 H₂O(s) →CuSO4(s) + 5 H₂O(g) If 4.06 g CuSO4 5 H₂O is decomposed to CuSO4, predict the mass of the remaining light blue solid.
How much energy is required to produce 11 grams of glucose (C6H12O6; 180 g/mol) from CO2 and H2O. Use the following combustion equation to help you answer the question? C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH=−2900kJ
A 1.50 g sample of pure sucrose is burned in a bomb calorimeter that has a heat capacity of 8.930 kJ/°C. The temperature of the water jacket rises from 24.00 °C to 26.77 °C. Incorrect. What is AE for the combustion of 1 mole of sucrose, C12H22O11? i ! kJ mol-1 Hint Assistance Used X Incorrect. How many dietary Calories per gram does sucrose provide when metabolized? Qu Nur i 39.28 ! Cal/g
© Macmilla The combustion of 1.524 g of sucrose, C12H22O₁₁ (s), in a bomb calorimeter with a heat capacity of 4.50 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.22 °C to 27.81 °C. What is the internal energy change, AU, for the combustion of 1.524 g of sucrose? AU = Calculate the enthalpy of combustion, AH, of sucrose in kilojoules per ΔΗ AH₁ = mole. kJ/mol kJ
3. Calcium sulfate is a byproduct of some types of oil extraction. Some companies process the calcium sulfate by extracting sulfur from it. The first step in this sequence is CaSO4(s) + CO(9) CaO(s) + SO2(g) + CO2(g) If you have 36kg of calcium sulfate to process, how much energy will be transferred? (Give the amount, and clearly state whether the energy is absorbed or released.)
When 0.515 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8oC to 29.4oC. Find ∆Erxn for the combustion of biphenyl in kJ/mol. The heat capacity of the bomb calorimeter, determined separately, is 5.86 kJ/C.
How many moles of hydrogen is consumed when 288 kJ of energy is released from the complete combustion of H2(g) in O2(g)? Do not include unit. Keep 2 decimal places in your answer. 2H2(g) + O2(g) → 2H2O(l); ΔrH° = –571.6 kJ/mol-rxn
How much energy in kJ is released in burning 2.5 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol) The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ) ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8 Round your answer to 2 decimal places.
Calculate the heat (kJ) exchanged when 3.76 mol CaCO3 is formed in the following reaction: Ca(OH)2 (s) + CO2 (g) → CaCO3 (s) + H2O (g); ΔH°rxn = −69.1 kJ Group of answer choices None of these choices is correct. −18 kJ −260 kJ −69 kJ −73 kJ
How much heat (in kilojoules) is evolved or absorbed in the reaction of 2.90 gg of Fe2O3Fe2O3 with enough carbon monoxide to produce iron metal?Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) ΔH∘Fe2O3(�)+3CO(�)→2Fe(�)+3CO2(�) Δ�∘ = -24.8kJkJ.
The following chemical reaction is exothermic releasing 283 KJ/mole of heat. CO(g) + ½O2(g) ⟷ CO2(g) How would you increase the amount of product produced from this reaction?