calculate the heat of reaction using Bond energy method for the complete combustion of buthane (C4H10). water vapour and carbon dioxide are produced in the reaction, include a thermal chemical equation. Colcalate the heat of reartion usina bond energy" method.for the wmplete cam bustion of buthane. water vapurOhnd carbon dioxide ore poduced ih the reaction, include ather mochemical equation.

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calculate the heat of reaction using Bond energy method for the complete combustion of buthane (C4H10). water vapour and carbon dioxide are produced in the reaction, include a thermal chemical equation

calculate the heat of reaction using Bond energy method for the complete combustion of buthane (C4H10). water vapour and carbon dioxide are produced in the reaction, include a thermal chemical equation

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...

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Students were asked to determine the heat of reaction forthe neutralization of a newly synthesized monoprotic acid HX and NaOH. Theyfirst calibrated the styro ball calorimeter using the reaction of 15.0 mL of 0.100 MHCl and 20.0 mL of 0.0500 M KOH. This recorded a change in temperature from26.5 °C to 31.8 °C. Afterwards, they determined the heat of reaction for a mixtureof 5.00 mL, 1.00 M NaOH and 10.0 mL, 1.00 M HX. This showed an increase intemperature of 3.6 °C.i. What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol)?ii. Write the balanced chemical and net ionic equations for the reaction of NaOHand HX .iii. What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH ?iv. Is the reaction between NaOH and HX endothermic or exothermic ?
b) Construct an enthalpy cycle and calculate the enthalpy of combustion in each case using the above data. 3. Given the following data: AH(CH4) = -74.8 kJmol-¹, AH(CH3CI) = -134.5 kJmol-¹, AH (HCI) = -92.3 kJmol-¹; Construct an enthalpy cycle and calculate H for the reaction CH4(g) + Cl2(g) CH3CI(g) + HCl(g) 4. Given the data: 4NH3(g) + 302(g) 0 2N2(g) + 6H2O(1), AH = -1530kJmol-1 H2(g) + 1/2O2(g) □ H₂O(1), AH = -288 kJmol-¹ Construct an enthalpy cycle and calculate the enthalpy of formation of ammonia.
2. Calculate the enthalpy change of the reaction that produces carbon monoxide by treating CO2 (g) with H2(g), under the reaction: CO2 (r) + H2 (,) > CO (g) + H2O (a) Use the standard enthalpies of formation for CO2 (g), CO (g) and H₂O (g) found on the chart provided. ind sare to interact with. Your Teedpack will help us improve
Phenol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard heat of combustion of phenol, CH,OH(s), is -3054 kJ/mol. Given that AHÇ [CO2(g)] = -393.5 kJ/mol and AHS [H,O(1)] = -285.8 kJ/mol, what is the standard %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A chunk of lead weighing 19.61 grams and originally at 97.01 °C is dropped into an insulated cup containing 82.14 grams of water at 21.79 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.61 J/°C.Using the accepted value for the specific heat of lead (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
Consider the following two-step reaction:C2H4(g) + Cl2 = C2H2Cl4(l) + H2(g) delta H = -385.76 kJ/mol C2H2Cl4(l) = C2HCl3(l) + HCl(g) Show that the overall reaction has standard heat equal to -421.017 kJ/mol using the heats of formation method.
determine the enthalpy change for each of the reactions: (It is necessary to draw Lewis structures so you know where there may be single, double or triple bonds) H2 + Br2 = 2HBr CH4 + I2 = CH3I + HI C2H4 + 3O2 = 2CO2 + 2H2O 2C2H6 + 7O2 = 4CO2 + 6H2O
Acetylene (CH2) is commonly used as a fuel for welding. a) Write a balanced chemical equation that describes the combustion of acetylene. b) Calculate AHrn for the combustion of 1 mole of acetylene. c) A steel MC cylinder can contain 310 grams of acetylene. Calculate the heat released by the combustion of the acetylene in 1 steel MC cylinder. d) How much water can you warm from 20 °C to 90 °C using 310 grams of acetylene. e) How much ice can you melt at 0 °C using 310 grams of acetylene.
Carbon disulfide, CS2, is a colorless, toxic, highly volatile, and flammable liquid. What is the heat of vaporization of CS,? CS: (1) - CS2 (9); AH =? AH;(CS (1)) = 89.7 kJ/mol AH;(CS (9)) = 116.9 kJ/mol Heat of vaporization - k)
An unknown organic compound is being proposed as an alternative to gasoline. The enthalpy of combustion of this compound is 208kcal mol-1. The density is 0.247g mL-1. The molecular weight of this compound is 315.82g mol-1. How much heat in kcal is released from combustion of 0.17 L of organic compound? Round your answer to 2 decimal places.