A styrofoam calorimeter contains 70.0 mL of 2.50 M NaOH at 20.3°C.When 10.28 g H₂C₂O is added to the calorimeter, the temperature of theresulting solution increases to a maximum of 44.7°C. The reaction that occurs is:H₂C₂O4(s) + 2 NaOH(aq) → Na₂C₂O4 (aq) + 2 H₂O(1)AH reactionreactionWhat is the (experimental) enthalpy change for this reaction, AH ? (Use the total mass ofsolution and 4.18 J/(g °C) for the specific heat of the solution in your calculations.)kJ/mol= = ???

Given reaction between oxalic acid and sodium hydroxide is as follows: H2C2O4(s)+2NaOH(aq) →…

A styrofoam calorimeter contains 70.0 mL of 2.50 M NaOH at 20.3°C. When 10.28 g H₂C₂O is added to the calorimeter, the temperature of the resulting solution increases to a maximum of 44.7°C. The reaction that occurs is: AH reaction H₂C₂O4(s) + 2 NaOH(aq) → Na₂C₂O4 (aq) + 2 H₂O(1) reaction What is the (experimental) enthalpy change for this reaction, AH ? (Use the total mass of solution and 4.18 J/(g °C) for the specific heat of the solution in your calculations.) kJ/mol = = ???

A styrofoam calorimeter contains 70.0 mL of 2.50 M NaOH at 20.3°C. When 10.28 g H₂C₂O is added to the calorimeter, the temperature of the resulting solution increases to a maximum of 44.7°C. The reaction that occurs is: AH reaction H₂C₂O4(s) + 2 NaOH(aq) → Na₂C₂O4 (aq) + 2 H₂O(1) reaction What is the (experimental) enthalpy change for this reaction, AH ? (Use the total mass of solution and 4.18 J/(g °C) for the specific heat of the solution in your calculations.) kJ/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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A chemist measures the enthalpy change AH during the following reaction: COC1₂(9) + 4 NH3(9)→ CO(NH₂),(s) + 2NH4Cl(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. esc COC₁₂ (8) + 2NH₂(g) → CO(NH₂), (s) + NH₂Cl(s) 1 1 ẩCO(NH,),() + ≈NH,C() → † COCI,(8) + NH, (8) CO(NH₂)₂ (s) + 2NH₂Cl(s) → COCL, (g) + 4NH, (g) Explanation THE Check reaction I > AH=-559. kJ Costa ΔΗ kJ ☐ kJ KJ MacBook Pro x10 X S © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc You MOSISO L
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10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
A 100.0-mL sample of 1.0 M NaOH is mixed with 50.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing is 22.3 °C. After the NaOH solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured is 31.4 °C. Assume that the density of the mixed solution is 1.00 g/mL, the specific heat of the mixed solutions is 4.18 J/g•°C, and no heat is lost to the surroundings.(a) Write a balanced chemical equation for the reaction that takes place.(b) Is there any unreacted NaOH or H2SO4 remaining after the reaction?(c) Calculate the enthalpy change per mole of H2SO4 in the reaction.
A 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.47oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)
Calculate AHO,xn for each of the following using data from Appendix B. (a) 2 H2S(g) + 3 02(g) → 2 SO2(g) + 2 H20(g) kJ (b) SiO2(s) + 4 HF(g) → SİF4(g) + 2 H20(/) kJ
Hydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine makes for an easily replaceable substituent, these bromine precursors are a necessary part of a vast amount of organic eynthesis, Calculate the reaction enthalpy for the synthesis of HBr according to H2(g) + Bra)2Br(g) Use the following information: NH3(g) +HBr(g) → NHABr(s) AH =-188.32 kJ Na(g) + 3H2(g) → 2NH3(g) AH = -92.22 kJ N2(g) + 4H2(g) + Br2(1) → 2NHABr(s) AH =-541.66 kJ a. AH =-728 kmol b. AH =-1010.52 KJjmol C. AH =-826.08 KJ/mol d. AH =728 kJ/mol e. AH = -257.24 kJ/mol Clear my choice
Coffee cup calorimetry experiments can be used to obtain DHfo for magnesium oxide. To determine the heat capacity of the calorimeter, 49.6 mL of 1.01M HCl are reacted with 50.1 mL of 0.998M NAOH: HCl(aq) + NaOH(aq)→NACI(aq) + H2O(1). The solution's temperature increases by 6.40 oC. Determine the heat capacity of the calorimeter. You may assume that the solution's specific heat is 4.025 J/g*oC and the enthalpy of neutralization is -55.9 kJ/mol of H2O. You may assume that the density of the solution is 1.00 g/mL.
A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC