Molar mass of acetone = 58.08 g/mol
Moles of acetone reacts = 2 mol
Mass of acetone reacts in reaction = moles * Molar mass = 2 mol * 58.08 g/mol = 116.16 g
Thus, 116.16 g of acetone reacts to produce 3571.5 kJ of heat
So, 21.49g of acetone reacts to produce 3571.5 kJ * 21.49 g/ 116.16 g = 660.74 kJ
Answer = 660.74 kJ
2C3H60 6) + 8020) - 6CO2 (g) + 6H20 (0) If AHpX = -3571.5 kJ, how...
Question 2 3 pts The heat of fusion for glycerol (C3H803) is 18.48 kJ/mol. How much heat would be absorbed when 227.57 g of glycerol undergo fusion? Express your answer in units of kilojoules (kJ) using at least three significant figures. Question 3 3 pts The Arxn for the combustion of acetone (C3HO) is -895 kJ, as shown below. How many grams of Oz would need to be consumed by this reaction in order to release 571.9 kJ of heat?...
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write the equilibrium constant expression for K. and for Kp, if appropriate, for the reaction. b. State whether the equilibrium is heterogeneous or homogeneous. c. State how the equilibrium would respond to the addition of some of the water from the system. d. State how the equilibrium would respond to a decrease in the partial pressure of ammonia (NHa). e. State how the equilibrium would...
For the following reaction: 2 CH. (g) + 702(g) → 4 CO2 (g) + 6H20 (1) AH° = -3119 kJ a) How much heat, in kJ, is associated with the combustion of 8.50 g of ethane? b) What is the quantity of work, in kJ, evolved in the combustion of 8.50 g of ethane at 25.00°C? (Assume an exact stoichiometric quantity of oxygen is present). c) Explain the significance of the sign of your answer in part (b) in one...
6. The heat of vaporization of ethanol, CH.0, is 38.56 kJ/mol, and it has a boiling point of 78.4°C. How much energy is released when 55.0 g of ethanol condenses? 7. 250 mL of room temperature water (22C) is placed in the freezer in an ice cube tray. If the freezer's temperature is -4.0°C, how much energy will it take to make ice?
Consider the following reaction: CO(g) + 2 H2(g) → CH2OH (9) AH = -90.7 kJ Calculate the amount of heat transferred when 107.3 g of CH2OH is synthesized by the above reaction at constant pressure. Select one: oa. -90.7 kJ ob. 9.732 x 102 kJ O C. 3.037 x 102 kJ O d. -3.037 x 102 kJ o e. 9.732 x 10 kJ Consider the following reaction: CO(g) + 2 H2 (g) → CH3OH (9) AH = -90.7 kJ For...
How much heat is released if 7.15 g Cao(s) is added to 152 g of H2O(l)?! Cao(s) + H2O) - Ca(OH)2(s) AHxn = -64.8 kJ/mol Select one: a. 7.68 kJ O b.8.26 kJ O c. 508 kJ d. 547 kJ O e. 555 kJ
Chapter 3, Question 21 Parameterization When 2.29 g of octanol ( C3H180 ) burns completely in excess O2 gas at constant pressure and 298 K, it releases -93.0 k) of energy. X Incorrect. Write the balanced chemical equation for this reaction. Ignore aggregation states in your answer. Edit X] Incorrect. (a) What is the molar energy of combustion (in kJ/mol) of octanol ? kJ/mol (b) How much energy (in kJ) is released per mole of Oz consumed?
Part A: Draw the Lewis structures of all the molecules involved in the reaction: N2(g)+3H2(g)→2NH3(g) Part B: If the bond energy for the N≡N bond is 946 kJ/mol, how much energy is needed to break all the bonds in 3.0 mol of nitrogen molecules? Part C: If the bond energy for the H−H bond is 432 kJ/mol, how much energy is needed to break all the bonds in 9 hydrogen gas? Part D: If the bond energy for the N=H...
A typical nuclear fission reaction involving uranium-235 produces 9.2 × 10 7 kJ/g of uranium. How much energy would be released if 1 mol of uranium-235 undergoes fission? A. 5.5 × 1021 kJ B. 3.9 × 105 kJ C. 9.2 × 107 kJ D. 2.2 × 1010 kJ
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