1) A bomb calorimeter containing 1.2 kg of water was used to evaluate the enthalpy of combustion of 2.0 g of benzoic acid (M.wt = 122g/mol) and the enthalpy (AH° rxn) of was found to be -3330 kJ/mol benzoic acid. During reaction the temperature of water raised from 25 °C to 28.5 °C If specific heat of water = 4.184 J/g.°C. Find the heat capacity of the calorimeter in kJ/°C

1) A bomb calorimeter containing 1.2 kg of water was used to evaluate the enthalpy of combustion of 2.0 g of benzoic acid (M.wt = 122g/mol) and the enthalpy (AH° rxn) of was found to be -3330 kJ/mol benzoic acid. During reaction the temperature of water raised from 25 °C to 28.5 °C If specific heat of water = 4.184 J/g.°C. Find the heat capacity of the calorimeter in kJ/°C

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...

See similar textbooks

Similar questions

a) Calculate the enthalpy variation produced in the butane combustion reaction under standard conditions.b) what amount of heat will be released in the complete combustion of the 12kg of butane contained in a cylinder dH standard CO2 (g) = -393kJ / mol, H2O (l) = -286kJ / mol, C4H10 (g) = -125kJ / mol
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 ?
Calculate the enthalpy change in kJ for the following reaction given the data below. Answer: -610.1 kJ P4O10(g) + 6 PCl5(g) --> 10 Cl3PO(g) A 1/4 P4(s) + 3/2 Cl2(g) --> PCl3(g) Ho/kJ = -306.4 B P4(s) + 5 O2(g) --> P4O10(g) Ho/kJ = -2967.3 C PCl3(g) + Cl2(g) --> PCl5(g) Ho/kJ = -84.2 D PCl3(g) + 1/2 O2(g) --> Cl3PO(g) Ho/kJ = -285.7
Calculate the change of enthalpy for the reaction 2AI (s) + 3C12 (g) --> 2AICI3 (s) from the following reactions: Reaction 1: 2AI (s) + 6HCI (aq) --> 2AICI3 (aq) + 3H2 (g) Change in enthalpy: -1049 kJ Reaction 2: HCI (g) --> HCI (aq) Change in enthalpy: -74.8 kJ/mol Reaction 3: H2 (g) + Cl2 (g) --> 2HCI (g) Change in enthalpy: -1845. kļ/mol Reaction 4: AICI3 (s) --> AICI3 (aq) Change in enthalpy: -323. kJ/mol Include the following: • The numerical answer with correct units. • State which reactions, if any, you had to "Flip". • State which reactions you had to multiply, if any, to get the correct amount of the compound.
Please help me solve the given question, explain and make sure its 100% correct ! Greatly appreciate it
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
Calculate the amount of heat released (absolute value) when 0.700 kg of liquid ethanol is burned in excess oxygen to make carbon dioxide and liquid water. The enthalpies of formation of the products and reactants are:CO2(g): -393.51 kJ/molH2O(l): -285.83 kJ/molO2(g): 0 kJ/molC2H5OH(l): -276.0 kJ/mol
Phenol undergoes combustion in oxygen to produce carbon dioxide gas and The standard heat of combustion of phenol, CgH,OH(s), is -3054 kJ/mol. AH?[CO,(g)] = -393.5 kJ/mol and AHÇ [H,O(1)] = -285.8 kJ/mol, what is t %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
Which equation from the formula bank is used to determine the experimental heat (q) in kJ involved when in a combustion reaction of 0.45 g of ethylene (MM = 28.00 g/mol) in an uninsulated device submerged in 100.0 mL of water (density 1.00 g/mL, s = 4.184 J/goC) where the temperature change (DT) is recorded as 12.5oC?
Please don't provide handwritten solution ....
(d) The enthalpy change for the reaction (A,Hº) of ethyne (C,H,) is -2511.6 kJ. i. Write a balance equation for the combustion of ethyne. ii. Determine the enthalpy of formation A¡Hº of ethyne given the following: A¢H° CO2 = -393-5 kJ mol" A¡Hº H2O_ = -241.8 kJ mol" A¡H° O2 = 0.00 kJ mol-1 %3D
do the highlighted question