The formula to calculate the heat is:
Where q is the heat, m is the mass, c is the heat capacity and delta T is the change in temperature.
In our system, we have a total of 2 L, which are equivalent to 2 kg, due to the density being 1.00 g/mL. c is also known and delta T is: 28.1 °C - 25.0 °C = 3.1 °C. So, the heat is:
This is the heat absorbed by the solution, which is the same as the heat released by the reaction, which has the same absolute value, but with a negative sign: -26.0 kJ.
C) 3400 D ) 2000 Q10: 1.0 L of 1 M NaOH(aq) and 1.0 L of 1 M HNO3(aq), both initially at 25.0 °C, were mixed in a calorimeter. The temperature of the solution increased to 31.1°C. Calculate the enthalpy of neutralization in KJ/mol)? Assume that the specific heat capacity of all solutions is 4.184 J/gºC, the density of all solution is 1.00 g/ml and that the calorimeter doesn't absorb any heat. A) -80.1 kJ/mol B) - 77.8 kJ/mol C)...
Enthalpy of Neutralization Reaction: A 25.0 mL sample of 0.200 M NaOH is mixed with a 25.0 mL sample of 0.200 M HNO3 in a coffee cup calorimeter. NaOH and HNO3 will undergo Neutralization Reaction according to the following balanced equation: NaOH(aq) + HNO3(aq) --> NaCl (aq) + H2O (l) Both solutions were initially at 35.00°C and Tmax of the resulting solution was recorded as 37.00°C (from the graph). Assume 1) that no heat is lost to the calorimeter or the surroundings, and...
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M NaOH in a coffee cup calorimeter. Assuming the temperature of the solution was initially 25.0 °C, and the final temperature of the solution was 26.7 °C, calculate the enthalpy of this reaction per mole of HCl. Assume the density of the water and acid and base solutions are all 1.00 g/mL.
When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of 0.700 mol/L HCl, both initially at 20.0 °C, the temperature increased to 22.1 °C. The heat capacity of the calorimeter is 279 J/°C. Since the solutions are mostly water, the solutions are assumed to have a density of 1.0 g/mL and a specific heat of 4.18 J/g°C. What is the mass of the solution? Select one: a. No enough information b. 50.0 g c. 50.0 kg d. 25.0...
TC01E03 25.0 mL of 1.00 M NaOH solution is mixed with 25.0 mL of 1.05 M HCl in an open calorimeter. You can assume volumes of these solutions are additive. The density of the resulting solution is 1.03 g/mL and its heat capacity is 3.90 J/K/g. The temperature of the calorimeter and its contents rose by 6.70 °C. What is the molar enthalpy of reaction for NaOH reacting with HCI? You can neglect the heat capacity of the calorimeter. Select...
Consider the following reaction. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) If 25.0 mL of a 0.100 M solution of NaOH reacted with excess HCl, how many moles of NaCl could form? a. 0.00250 mol b. 0.100 mol c. 25.0 mol d. 2.50 mol 1 points QUESTION 9 Consider the following reaction. How many grams of sucrose would produce 2546 kcal? a. 649.4 g b. 1342 g c. 180.4 g d. 1.897 g
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/oC....
100 mL of 0.500 M HCl is mixed with 100 mL of 0.600 M NaOH in a constant pressure calorimeter. The initial temperature of the solutions is 22.50 C and the final temperature of the mixed solution is 25.86 C. Calculate ?rH (in units of JK/mol-rxn) for the reaction NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) The density of the resulting solution is 100 g/mL, and its specific heat is 4.184 J/(g C). Thank you in advance!
HCl and NaOH react according to the following equation: HCl (aq) + NaOH → Na+(aq) + Cl-(aq) + H2O(l) In a coffee cup calorimeter, 50mL of 2.00 M HCl was combined with 50mL of 2.05 M NaOH. The temperature of the solution rises from 22 degree C to 36 degrees C. What is the enthalpy change for the reaction (delta H rxn)? What is the molar enthalpy for the reaction? Given: The heat capacity of the calorimeter (Cc) is 14.0...
1. How many milliliters of 0.112 M Na2CO3 will completely react with 27.2 mL of 0.135 M HNO3 according to the reaction 2HNO3(aq) + Na2CO3(aq) → H2O(l) + CO2(g) + 2NaNO3(aq) Part B.) A 25.0-mL sample of HNO3 solution requires 35.7 mL of 0.108 M Na2CO3 to completely react with all of the HNO3 in the solution. What is the concentration of theHNO3 solution? Part C.)Consider the reaction HCl(aq) + NaOH(aq) → NaOH(aq) + H2O(l) How much 0.113 M NaOH...