Calculate the lower calorific value of acoal sample having the followingcompositions: C=72%, H=8%, O3D7%,N=6.5%, ash=4.5%, S=2%. Latent heat ofSteam = 587 cal/g.O 8,276 kcal/g8,301 kcal/gO 8,723 kcal/gO 8,504 kcal/g

Lower calorific value is the amount of heat evolved when unit mass. It is also called as net…

Calculate the lower calorific value of a coal sample having the following compositions: C=D72%, H=8%, 03D7%, N=6.5%, ash=4.5%, S=2%. Latent heat of steam = 587 cal/g. O 8,276 kcal/g 8,301 kcal/g O 8,723 kcal/g O 8,504 kcal/g

Calculate the lower calorific value of a coal sample having the following compositions: C=D72%, H=8%, 03D7%, N=6.5%, ash=4.5%, S=2%. Latent heat of steam = 587 cal/g. O 8,276 kcal/g 8,301 kcal/g O 8,723 kcal/g O 8,504 kcal/g

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.76P

See similar textbooks

Similar questions

A group of Chem 16.1 students was 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. What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH? Determine if the reaction between NaOH and HX is endothermic or exothermic.
The enthalpy of neutralization of a newly discovered compound, J(OH)3, was determined using a styroball calorimeter. The calorimeter was first calibrated using 13.00 mL of 0.104 M NaOH and 11.29 mL of 0.125 M HCl (ΔH = -55.85 kJ/mol) and a temperature rise of 4.6 °C was recorded. Using the same calorimeter, 7.58 mL of 0.151 M of J(OH)3 was reacted with 9.60 mL of 0.125 M HCl and the temperature changed from 25.9 °C to 23.4 °C. a. What is the heat capacity of the calorimeter? b. Write the balanced chemical equation for the reaction between J(OH)3 and HCl.c. Identify the limiting reactant in the reaction between J(OH)3 and HCl. d. What is the enthalpy of the reaction of J(OH)3 and HCl?
A group of Chemistry students was 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. What is the heat capacity of the calorimeter in J/℃ (∆??????????????? =-55.85kJ/mol)?
A coffee cup calorimeter was calibrated using 5.01 mL of 0.901 M HCl and 10.01 mL of 0.751 M NaOH. Thereafter, T changed from 29.5oC to 32.5oC. Using the same calorimeter, the enthalpy of reaction between NaOH and HNO3 is determined by mixing 5.10 mL of 0.800 M HNO3 and 10.10 mL of 0.600 M NaOH. The T changed from 30.5oC to 32.5oC. Suppose that the delta H of reaction between H+ and OH- is -55.9 kJ/mol. i. Find the heat capacity of the calorimeter and the limiting reactant of the reaction studied. ii. Find qrxn and enthalpyexperimental of the reaction. iii. Find the % error.
A coffee-cup calorimeter was calibrated using 10.0 mL of 0.100 M HCl and 2.00 mL of 0.300 M NaOH (ΔHoneutralization= -55.8 kJ/mol). The reaction mixture had 0.300oC increase in temperature. Using the same calorimeter, 5.00 mL of 0.250 M HNO3 was made to react with 7.00 mL of 0.100 M NaOH. A temperature rise of 0.320o C was observed. What is the ΔHoreaction of this reaction? Select one: a.~ –51.0 kJ/mol b.~ +55.8 kJ/mol c.~ +51.0 kJ/mol d.~ –35.8 kJ/mol
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.…
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 ?
A group of students was 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. 1.) What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol) 2.) Write the balanced chemical and net ionic equations for the reaction of NaOHand HX
A group of students was 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. 1.) What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol) 2.) Write the balanced chemical and net ionic equations for the reaction of NaOHand HX 3.) What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH? 4.) Is the reaction between NaOH and HX endothermic or exothermic?
Please answer the following question: The combustion of isoctane reaction produces -5099.5 kJ of heat per mole of C8H18(g) consumed, under standard conditons. The enthalpy of formation (DHf) for CO2(g) and H2O(g) are -393.5 kJ/mol and -241.8 kJ/mol, repspectively. Find the standard enthalpy of formation (DHf) of this isomer of C8H18(g)? (Show work) C8H18(g) + O2(g) -> 8CO2(g) + 9H2O(g) DHrxn = -5099.5 kJ