A 104.2 mL sample of 1.00 M NaOH is mixed with 52.1 ml of 1.00 MH2SO, in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.05°C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.90 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g°C), and that no heat is lost to the surroundings. 1st attempt Part 11 E See Periodic Table Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. He (ag). Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. He Part 2 Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over? Choose one: O A. Yes O B. No O See Hir Part 3- Calculate the enthalpy change per mole of H2SO, in the reaction. kJ/mol

A 104.2 mL sample of 1.00 M NaOH is mixed with 52.1 ml of 1.00 MH2SO, in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.05°C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.90 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g°C), and that no heat is lost to the surroundings. 1st attempt Part 11 E See Periodic Table Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. He (ag). Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. He Part 2 Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over? Choose one: O A. Yes O B. No O See Hir Part 3- Calculate the enthalpy change per mole of H2SO, in the reaction. 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. Directions: Solve the following problem using the thermochemical equation. Write your answer on your answer sheet. 1. Using the following thermochemical equation, calculate how much heat is associated with the decomposition of 4 mol of NH.CI. NHJ + HCl - NH.Cl AH- -176 kJ 2. How many grams of Na are needed to make -550.0 kJ? Naw+ 3Ha + 2NHs AH - -92.6 kJ 3. Calculate the mass of ethane, CaHo which must be burned to produce 100 KJ of heat. 2C,Heg + 70ag - 4CO2g + 6H,O AH - -3120 KJ B. Calculate the enthalpy change of the reaction using Hess's Law. Write your answer on your answer sheet. 1. Calculate AH for the reaction CaHag + Ha -->C:Hoog, from the following data. C,Ha + 30a - 2COa + 2H,Om C;Hoe + 7/20a - 200a + 3H,O Hag + 1/20z - H20 AH - -1411. kJ/mole AH - -1560. kJ/mole AH - -285.8 kJ/mole 2. Calculate AH for the reaction 4NH3 + 50z0 - 4NO + 6H2O, from the following data. Na + Oz - 2NO Naw + 3Ha - 2NH 2Hay + Oz + 2H20 AH - -180.5 kJ/mole AH - -91.8 kJ/mole AH - -483.6 kJ/mole 3.…
To calibrate a calorimeter, 10.0 ml of 1.0 M NaOH and 5.0 ml of 1.0 M HCl was used in a calorimetry experiment. Which of the following will have NO EFFECT on the calculated heat capacity of the calorimeter, Ccal? a. Accidentally adding HNO3 instead of HCl. b.Adding a smaller volume of 1.0 M HCl. c.Using a bigger styrofoam ball for calibration. d.Using a wet test tube for calibration.
What is the enthalpy change, Delta Hrxn, for the following reaction? 2 RbI (s) + Cl2 (g) --> 2 RbCl (s) + I2 (s) a. 1.33 x 103 kJ b. 656 kJ c. – 215 kJ d. 107 kJ e. 763 kJ f. none of these g. – 1.33 x 103 kJ h. 871 kJ
pt pt pt pt pt pt pt pt pt pt pt pt pt pt You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.8 g of concentrated H₂SO4() was added (with stirring) to 140. g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 21.0 °C to 30.3 °C. Calculate the enthalpy change for the process H₂SO4(l) → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change = kJ/mol ?
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ature of a 12.58 g sample of calcium carbonate [CaCO,(s)] decreases from 382 C to 23.6 C the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are lost to the surroundings? Select one: O a. 151 O b. 7.5 OC.-5.0 O d. -0.82 e. -138
A calorimeter contains 100 g water. The calorimeter and the water inside are both at 21 °C. What mass of hot water 95 °C must be added to raise the temperature inside the calorimeter to 36 °C ? (Assume no heat leaks). calorimeter constant: 150 j°C1 specific heat of water: 4.184 J°c-1g-1 51.5 g Oa. Ob. 29.5 g O. 34.5 g O d. 42.5 g O e. 19.5 g A Moving to the next question prevents changes to this answer. Question 11 of 20 >
59.8 J was required to raise the temperature of 25.0 g of ethylene glycol by 1.00 K. Calculate the specific heat capacity of ethylene glycol. O a. 2.39 J/g.K O b. None of the above O c. 2.03 J/g.K O d. 1.39 J/g.K Next page Documents Jump to...
Calculate the energy content (in calories) of a 1.00 g of product that is placed inside a calorimeter having a heat capacity of 950 J/K. Data from the calorimeter indicated that the 3.0 L surrounding water had initial and final temperatures of 18.0 °C and 47.5 °C, respectively. Specific heat capacity of water: 4.18 J/g-K a. 2.6x10^4 cal b. 9.5x10^4 cal c. 8.8x10^4 cal d. 7.3x10^4 cal
SUBJECT : GENERAL CHEMISTRY 2 TOPIC : HEAT AND CALORIMETRY
6. What is the energy required to raise the temperature of 22.0 g of water from 15.0 °C to 20.0 °C? a. 110J b. 18.4 J c. 26.3 J d. 460 J