Suppose 200.0 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH, both initially at 25.0°C, are mixed in a thermos flask. When the reaction is complete, the temperature is 28.4°C. Assuming that the solutions have the same heat capacity as pure water, compute the heat released (in kJ).

THe G.R.A.S.P. method

Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJ

When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)

In a coffee cup calorimeter, a student places 0.350 g of magnesium, followed by addition of 45.0 mL of 1.00 M hydrochloric acid. After the reaction took place, a the temperature rose from 21.5oC to 54.2oC. If the reaction solution has the same properties of water and the calorimeter constant is 5.38 J oC-1, how much heat was released from the reaction and what is the enthalpy of the reaction in kJ mol-1? Answer choices for heat released from reaction: -7.89 kJ, -4.12 kJ, -6.50 kJ, -5.66 kJ

The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature. Note the difference between the terms molar heat capacity, which has units of J/(mol-K). and specific heat, which has units of J/(g-K). Remember to use 3 significant figures for all answers unless stated otherwise in the problem. Common issues with this problem involve entering units incorrectly into the answer field. Please check this help website for a refresher on how to enter units in Mastering Chemistry: http://help.pearsoncmg.com/mastering/student/standalone/TopicsStudent/acceptable units list.htm The margin of error is 2%. Part A A volume of 75.0 mL of H₂O is initially at room temperature (22.0 °C). A chilled steel rod at 2.00 °C is placed…

A student followed the procedure in this experiment , using 29.5 mL of 2.41 molar HCl and 31.5 mL of 2.41 molar NaOH , with both solutions having an initial temperature of 21.9 °C. After mixing , a maximum temperature of 31.0 °C is measured . The final mass of the mixture was found to be 62.201 grams . For this problem , assume the specific heat of the solution is 4.18 J/g °C. What is the heat transferred by this reaction, in Joules?

Use the References to access important values if needed for this question. A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity. When 6.36 g of KBr(s) is dissolved in 115.00 g of water, the temperature of the solution drops from 25.00 to 22.71 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AHdissolution = kJ/mol Submit Answer 5 question attempts remaining

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