In the following reaction, What quantity in moles of CH;OH are required to give off 1501 kJ of heat? 2 CH;OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H20(g) AH° = -1280. kJ
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- At constant pressure and 25°C, what is ΔrH° for the following reaction2C2H6(g) + 7O2(g) → 4CO2(g) + H2O(l)if the complete consumption of 14.5 g of C2H6 liberates 752.3 kJ of heat energy?At constant pressure and 25^C, What is delta H for the following reaction. 2C2H6(g) + 7O2(g) = 4CO2(g) + H2O(l) if the complete consumption of 38.2 g of C2H6 libraties 1981 KJ of heat energy?5. Provide an explanation for why the mixing acetone and cyclohexane is endothermic. How is this consistent with the sign of ΔVmix?
- When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…Carla and her friends were tasked with determining the heat of reaction for the neutralization of the newly synthesized monoprotic acid HX and NaOH. The rubber ball calorimeter was initially calibrated using the reaction of 7.0 mL of 0.200 M HCl and 14.0 mL of 0.1000 M KOH. This measured a temperature rise from 15.7 °C to 27.9 °C. After that, the heat of reaction was calculated for a combination of 2.00 mL of 1.00 M NaOH and 5.0 mL of 1.00 M HX. This represented a temperature rise of 3.7 degrees Celsius. What is the calorimeter's heat capacity in J/°C? (Δ??????????????? =-55.85 kJ/mol)? For the reaction between NaOH and HX, create the chemical and net ionic equations that are equally balanced.
- Carla and her friends were tasked with determining the heat of reaction for the neutralization of the newly synthesized monoprotic acid HX and NaOH. The rubber ball calorimeter was initially calibrated using the reaction of 7.0 mL of 0.200 M HCl and 14.0 mL of 0.1000 M KOH. This measured a temperature rise from 15.7 °C to 27.9 °C. After that, the heat of reaction was calculated for a combination of 2.00 mL of 1.00 M NaOH and 5.0 mL of 1.00 M HX. This represented a temperature rise of 3.7 degrees Celsius. The neutralization reaction between HX and NaOH has an experimental enthalpy of (in kJ/mol). What is this? Is the reaction between NaOH and HX endothermic or exothermic?Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. If qH2O = -910 J and qcal = -130 J for 5.0 g of NH4NO3, calculate the heat of solution in J per gram of NH4NO3.The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
- What is the enthalpy change when 175 g of C3H8 are burned in excess O2?C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(l) H = -2220 kJa. -1.71 107 kJb. -1.79 10-3 kJc. -3.47 100 kJd. -3.89 105 kJe. -8.83 103 kJYou place 5.82 g of a liquid PEG sample at 20.5 oC into a thermally-insulated container having 54.7 g water at the same temperature, and record the final equilibrium (plateau) temperature 44.9 oC. The specific heat of water is 1.00 cal/g/oC and the specific heat of PEG is 0.498 cal/g/oC. Calculate the hydration energy (heat of hydration) for PEG in units of kcal/g (careful!). Enter the value (do not enter units) to 3 significant figures.3. A 25.00 gram sample of barium chloride was dissolved in 75.00 grams of water. If the calorimeter constant, KCal, is 120 J/oC, how much heat is produced by the dissolution (absorbed from the solution) if the temperature goes from 18.00 oC to 0.55 oC. Assume the specific heat of the solution is 4.18 J/g oC.
