AHºrn and the Standard Enthalpies of Formation; Read Section 7.9. You can click on the Review link to access the section in your e Text. In making wine, glucose (C6H12O6) is fermented to produce ethanol (C₂H5OH) and carbon dioxide. The standard heat of formation of C6H12O6 (s) is - 1273.3 kJ/mol, that of CO2 (g) is -393.5 kJ/mol, and that of C₂H5OH(1) is -277.6 kJ/mol. Enter a balanced equation for alcohol fermentation. Express your answer as a chemical equation including phases. xa Submit ΑΣΦ Part B Xb a b a A chemical reaction does not occur for this question. x Request Answer X Calculate AHxn. Express your answer in kilojoules to one decimal place. 15| ΑΣΦ | ? ?

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

Use the References to access important values if needed for this question. A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity. When 6.36 g of KBr(s) is dissolved in 115.00 g of water, the temperature of the solution drops from 25.00 to 22.71 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AHdissolution = kJ/mol Submit Answer 5 question attempts remaining

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboard or In the laboratory a general chemistry student finds that when 3.38 g of CuCl,(s) are Styrofoam lid dissolved in 114.10 g of water, the temperature of the solution increases from 25.37 to 27.99 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C. Nested Styrofoam cups Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in kJ/mol. - Reaction occurs in Assume the specific heat of the solution is equal to the specific heat of water. solution. AHdissolution kJ/mol kc Cengage Ln

A 10.0-g sample of ammonium nitrate, NH4NO3, is added to 100.0 mL of water (density = 1.00 g/mL) in a Styrofoam calorimeter. The initial temperature of water and calorimeter is 25.0 oC. When the solid completely dissolves, the final temperature of the solution is 18.4 oC. (a) Calculate heat lost by water and by the calorimeter. (Heat capacity of calorimeter is 15 J/oC and the specific heat of water is 4.184 J/g.oC)(b) What is the total amount of heat (in Joules) absorbed by the system (the dissolution of solid NH4NO3). (c) Write an equation for the dissolution of NH4NO3(s) and calculate its molar enthalpy of dissolution, Hdissol. expressed in kJ/mol.

1. How much energy (in kJ) is required to change the temperature of 1.00 kg Fe from 25.0 °C to 1515 °C? The specific heat capacity of iron is 0.449 J/g·C.   2. MgO reacts with water to form Mg(OH)2. If 5.00 g MgO is combined with 100.0 g H2O in a coffee cup calorimeter, the temperature of the resulting solution increases from 22.3 °C to 32.9 °C. Calculate the enthalpy change (kJ) for the reaction per mole of MgO. Assume that the specific heat capacity of the solution is 4.18 J/g·C.   3. Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 25.69 kJ of heat per mole dissolved in water. In a coffee-cup calorimeter, 3.40 g NH4NO3 is dissolved in 100.0 g of water at 21.0 °C. What is the final temperature of the solution?  Assume that the solution has a specific heat capacity of 4.18 J/g·C

The combustion of hydrogen-oxygen mixtures is used to produce very high temperatures (ca. 2500 °C) needed for certain types of welding operations. Consider the reaction to be H₂(g) + ½O₂(g) → H₂O(g) ∆H° = -241.8 kJ/mol What is the quantity of heat evolved, in kilojoules, when a 180 g mixture containing equal parts of H₂ and O₂ by mass is burned?