What is the calorimeter constant in this experiment (exp.1) HelpLast edit was seconds agoBIUAO回因.11三ニ =▼=4.6.Added 45g water to 150ml flask. Initial temp =21.5CPlaced flask in a constant temp. bath at 60 degrees C.Added 45g of water to calorimeter while flask was in constant temp bath. Initialtemp=21.5C• Temp of the flask in constant temp bath reached 60 degrees C. Poured water contentsfrom the flask in constant temp bath into the calorimeter.Combined temp of both -41.5CExp. 2 Determine the Enthalpy of Neutralization of HCi by NH3Temp of empty calorimeter= 21.5C calorimeter zerned gut on scale!!lili

Heat energy absorbed or released in any process is given by Q = m c (T2-T1) where, Q = heat energy,…

Added 45g water to 150ml flask. Initial temp =21.5C Placed flask in a constant temp. bath at 60 degrees C. Added 45g of water to calorimeter while flask was in constant temp bath. Initial temp321.5C Temp of the flask in constant temp bath reached 60 degrees C. Poured water contents from the flask in constant temp bath into the calorimeter. Combined temp of both =41.5C

Added 45g water to 150ml flask. Initial temp =21.5C Placed flask in a constant temp. bath at 60 degrees C. Added 45g of water to calorimeter while flask was in constant temp bath. Initial temp321.5C Temp of the flask in constant temp bath reached 60 degrees C. Poured water contents from the flask in constant temp bath into the calorimeter. Combined temp of both =41.5C

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.94PAE

See similar textbooks

Similar questions

The formulas give the enthalpy when Coal and Methane react with oxygen:C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJCH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4gives 44 gram of CO2+891kJ 1-Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg.Calculate the lower heating value for Methane. 2-Calculate the amount of CO2 which is produced per kWh for Coal and Methane
Part B Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 gg of sucrose, C12H22O11C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘CkJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C∘C. Calculate the change in internal energy, ΔEΔEDelta E, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
hexane heptane ΔΗ°comb (kJ/mol) -4163.0 -4817.0 Liquid Denisty (g/mL) 0.493 0.684 By how much are the fuel values different? Give the magnitude of the difference (the absolute value). kJ/mL
In this calorimetery experiment state the independent variable, dependent variable, and your control group. Here is rhe procedure of the experiment below: Gather the items to set up your calorimeter (coffee-cup, stir plate and stir bar, Vernier temperature probe, lid for coffee-cup) Pour 50.0 mL of DI water into the coffee-cup calorimeter. You will be preparing 50.0 mL of a 1.0 M solution of sodium nitrate solution. Using the Vernier temperature probe, record the initial temperature of your DI water. Weigh out the mass of sodium nitrate (4.25g) needed for your solution and pour it into the calorimeter. Immediately begin collecting temperature data. Repeat multiple times.
Calculations for the Specidfic Heat for an Unknown Metal Trial 1 Trial 2 Mass of unknown metal(g) 18.371 18.371 Mass of calorimeter cup(g) 1.891 1.891 mass of calorimeter and water(g) 47.231 46.502 Tempature of boiling water bath (C) 98.50 99.2 Initial tempature of calorimeter water(C) 23.5 23.4 Final Tempature of water and metal(C) 24.8 24.8 Mass of water(g) Tempature change of water(C) (Do not include a negative sign) Heat gained by water (cal) (do not include negative sign) heat lost by metal(cal) (do not include negative sign) tempatire change of metal(C) (do not include negative sign) Specific heat of metal [cal/g. C] Specific heat of metal [J/(g. C)] Average specific heat of metal [J/(g·°C)] Identify the Metal based on the average specific heat in J/(g·°C)
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)?
Chemistry Calculate the heat capacity of 2.00 L of water, given the specific heat of water is 4.187 kJ kg-1K-1. Calculate the percent difference between this value and the mean of the bomb calorimeter’s heat capacity of 10.00 KJ/K. Was the water a large contributor to the overall Cv?
500.0 mL of 0.100 mol·L HCl(aq) was added to a high quality insulated calorimeter containing 500.0 mL of 0.100 mol·LNaOH(aq). Both solutions had a density of 1.000 g·mL and a specific heat of 4.184 J·g ·K . The calorimeter had a heatcapacity of 850.0 J·K . The temperature of the entire system rose from 25.50 C to 26.05 C.Calculate the heat of reaction. Thank you!
Given the following data in KJmol-1 C2H5OH(I) + 302(g)→2C02(8)+ 3H20(I) AH[] = -1370 C2H4 (g) + 302 (g)→ 2CO2 (g) + 2H2O(i) AH[] = -1415.6Determine the enthalpy change when 30.8g of ethanol is produced from the reaction below; C2H4 (g) + H2O(i) → C2 H5OH (i) (RMM of ethanol = 46).
2N2(g) + 3O2(g) ® 2N2O3(g) (delta)H°rxn = +86.6 kJ Consider a reaction mixture of 13 grams of 7N and 17 liters at STP (LSTP) of O2: … If all 13 grams of 7N react, the reaction heat is: _________ kJ … If all 17 LSTP of O2 react, the reaction heat is: _________ kJ … The limiting reagent in this mixture is _____ … The theoretical heat of this reaction mixture is: _______ kJ
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.
2C8H18(l) + 25 O2(g) = 16 CO2(g) + 18 H2O(l) The standard enthalpy of formation for H2O(g)is −241.82kJ/mol The standard enthalpy of formation for CO2(g)is −393.5kJ/mol The standard enthalpy of formation for C8H18(l) is −249.9kJ/mol 1)how much CO2 is released from 1 tank of gas? 2) there are 3000 students and employees. Further assume that they all drive, and on an average they consume 1 tank of gas each, every week to get to and from work. If every tank is 12 gallons (1 gallon = 3.785 L) can you estimate how much heat is transferred