You combine 25.0 mL 2.00 M HCl with the same volume of 2.00 M NaOH in a calorimeter. The temperature of the calorimeter rises by 12.5°C. What is the calorimeter's heat capacity, Ccal, in kJ/°C? Enter the numerical value to 3 significant figures, without units. (ΔH° for the neutralization of one mole of strong acid is -55.8 kJ.). For a particular reaction at 25.0°C, ΔG°= 19.2 kJ and ΔH° = 13.7 kJ. What is ΔS° for this reaction, in J/K? Enter the numerical value to 3 significant figures, without units.
You combine 25.0 mL 2.00 M HCl with the same volume of 2.00 M NaOH in...
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...
A common laboratory reaction is the neutralization of an acid with a base. When 41.2 mL of 0.500 M HCl at 25.0°C is added to 53.7 mL of 0.500 M NaOH at 25.0°C in a coffee cup calorimeter (with a negligible heat capacity), the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of NaCl (in kJ/mol)? Assume the mixture has a specific heat capacity of 4.18 J/(g·K) and that the densities of the...
A 48.53 mL volume of 1.00 M HCl was mixed with 47.70 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 26.0 J/°C) at 21.43 °C. The final temperature of the aqueous solution after the reaction was 29.71 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The total mass of aqueous solution inside the calorimeter (dsoln = 1.00 g/mL) g b. The change in temperature (∆T) of...
2. A 49.45 mL volume of 1.00 M HCl was mixed with 49.14 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.1 J/°C) at 21.34 °C. The final temperature of the aqueous solution after the reaction was 29.37 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: e. The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) e. The enthalpy...
A
calorimeter contains 25.0 mL of 0.300M X at 22.00C. To this, 75.0
mL of 0.100M Y (at 22.00C) is added.
The final temperature was found to be 20.00C. The calorimeter
constant is 25.0 J/K.
The reaction that occurs is: 2 X(aq) + Y(aq) = Z(s)
1) For the actual reaction, delta H = ? J [three significant
figures]
2) The thermochemical equation, which involves 2 moles of X
and 1 mole of Y per mole of reaction, is: 2...
2. A 49.21 mL volume of 1.00 M HCl was mixed with 48.05 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.6 J/°C) at 20.32 °C. The final temperature of the aqueous solution after the reaction was 29.83 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The total mass of aqueous solution inside the calorimeter (dsoln = 1.00 g/mL) g correct 1/1 b. The change in...
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...
Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.245 gram piece of metal and combine it with 58.7 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 42.75 g/mol, and you measure that the reaction absorbed 160 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...
Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.202 gram piece of metal and combine it with 76.3 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 48.37 g/mol, and you measure that the reaction absorbed 121 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...
Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.296 gram piece of metal and combine it with 57.5 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 50.61 g/mol, and you measure that the reaction absorbed 164 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...