Chemistry f) Glucose is the primary sugar in your bloodstream, supplying energy to your body. Dieticians are therefore very interested in the energy resource that it represents and need to investigate the enthalpy changes that accompany its reactions. A constant-volume calorimeter showed that the heat generated by the combustion of 1.000 mol glucose molecules in the reaction C6H12O6(s) + 60₂(g) 6CO2(g) + H₂O(g) is 2559 kJ at 298 K, AE = -2559 kJ. What is the change in enthalpy for the same reaction? (R-8.314J/K/mol).

Chemistry f) Glucose is the primary sugar in your bloodstream, supplying energy to your body. Dieticians are therefore very interested in the energy resource that it represents and need to investigate the enthalpy changes that accompany its reactions. A constant-volume calorimeter showed that the heat generated by the combustion of 1.000 mol glucose molecules in the reaction C6H12O6(s) + 60₂(g) 6CO2(g) + H₂O(g) is 2559 kJ at 298 K, AE = -2559 kJ. What is the change in enthalpy for the same reaction? (R-8.314J/K/mol).

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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2) A0.500 g sample of Trinitrotoluene (C7H$N2O6) is burned in a bomb calorimeter containing 610 grams of water at an initial temperature of 20°C. The heat capacity of the calorimeter is 420 J°C and the heat of combustion of Trinitrotoluene is 3374 kJ/mol. Using these data, calculate the final temperature of the water and calorimeter once the reaction is complete.
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 5.26 g of CsClO4(s) are dissolved in 103.30 g of water, the temperature of the solution drops from 22.98 to 19.81 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.
Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g) →C₂H₂(g) AH = -125.6 kJ (2) C₂H₂(g)2C(s) + H₂(g) AH = -226.7 kJ what is the standard enthalpy change for the reaction: (3) 2C₂H₂(g) + 3H₂(g)-CH₁0(g) AH° = ?
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(b) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 JgC and 0.3847 Jg l°C-' respectively.
What is the enthalpy change when 2.00 mol of oxygen (O2) react? C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(l) ΔH = -5644 kJ
When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ
The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C