A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes. The acid-base reaction is as follows: 2 NaOH(aq) + H2SO4(aq) ? Na2SO4(aq) + 2 H2O(l) The temperature of each solution before mixing is 22.3 °C. After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C. Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g·°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction. +85.6 kJ/mol -85.6 kJ/mol +5.71 kJ/mol -5.71 kJ/mol -114 kJ/mol
Added by Omar N.
Close
Step 1
We can use the formula: q = mcΔT where q is the heat, m is the mass of the solution, c is the specific heat capacity, and ΔT is the change in temperature. The total volume of the solution is 100.0 mL + 50.0 mL = 150.0 mL. Since the density is 1.00 g/mL, the Show more…
Show all steps
Your feedback will help us improve your experience
Snehal J and 81 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Sri K.
A 93.2 mL sample of 1.00 M NaOH is mixed with 46.6 mL of 1.00 M H2SO4 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 21.25 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.70 °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. Calculate the enthalpy change per mole of H2SO4 in the reaction.
A 100.0 mL sample of 1.0 M NaOH is mixed with 50.0 mL of 1.0 M H2SO4 in a coffee cup calorimeter. Each solution has a temperature of 22.3 °C before mixing. After addition of the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature is found to be 31.4 °C. Assume that no heat is lost to the surroundings, the density of all the solutions is 1.00 g/mL, and their specific heat is 4.184 J g-1 °C-1. a. Write a balanced chemical equation for the reaction that takes place. b. Calculate the enthalpy of the reaction per mole H2SO4 in the reaction.
David C.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Watch the video solution with this free unlock.
EMAIL
PASSWORD