Homework Answers
. A) 1.25 L B) 2.50 L Q13. 1.0 L of 1 M NaOH(aq) and 1.0...
. A) 1.25 L B) 2.50 L Q13. 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 calorimeter. The temperature of the solution rose to 28.1°C. How much heat was released? Assume the specific heat capacity of all solutions is 4.184J/(g°C), and the density of all solution is 1.00 g/l A)-80.1 kJ B) -77.8 C)-52.0 l D) -26,0 11
Enthalpy of Neutralization Reaction: A 25.0 mL sample of 0.200 M NaOH is mixed with a...
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...
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) → NaCN(aq) + H20(1)....
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) → NaCN(aq) + H20(1). Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH. If the temperature of the calorimeter increases by 2.58 °C, what is the enthalpy of this neutralization reaction (in kJ/mol)? Assume the density of the solution is 1.00g/mL and that the specific heat is...
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below HX(aq)+ NaOH(aq) NaCN(aq)+ H20(1) S...
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below HX(aq)+ NaOH(aq) NaCN(aq)+ H20(1) Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH If the temperature of the calorimeter increases by 2.02 C, what is the enthalpy of this neutralization reaction (in kJ/mol)? Assume the density of the solution is 1.00g/mL and that the specific heat is 4.184 J/g "C...
When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of...
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. What is the enthalpy of neutralization in kJ/ mole of HCl? 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. Select one: a. −1020 b. -58.6 c. −5856 d. 58.6
The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M...
The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 °C, and the final temperature after addition is 26.8 °c. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the...
Ferminow.com QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq)...
Ferminow.com QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) NaCN(aq) + H2O(l). Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50,0 mL of 0.500 M NaOH. If the temperature of the calorimeter increases by 1.91 °C, what is the enthalpy of this neutralization reaction (in kJ/mol? Assume the density of the solution is 1.00g/mL and that the specific heat is...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH" (aq) - H20 (1) is -56.2...
help 2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL...
help
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC. the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH(aq) → H20 (1) is -56.2...
i need help on the second page: "calculate how many mols of HCL you used based...
i need help on the second page:
"calculate how many mols of HCL you used based on the volume
and molarity of the HCL"
and
"enthalpy of reaction" parts
Part B Heat of Reaction for HCl(aq) + NaOH (aq) NaCl (aq) + so H20 (1) Volume of 1.0 M HCl (ml) so 100 23.3 Volume of 1.0 M NaOH (ml) Mass of Solution (8) use 1.00 g/ml Ti solution (temp of HCl just before reaction) T solution (highest temp obtained)...
. A) 1.25 L B) 2.50 L Q13. 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 calorimeter. The temperature of the solution rose to 28.1°C. How much heat was released? Assume the specific heat capacity of all solutions is 4.184J/(g°C), and the density of all solution is 1.00 g/l A)-80.1 kJ B) -77.8 C)-52.0 l D) -26,0 11
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) → NaCN(aq) + H20(1). Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH. If the temperature of the calorimeter increases by 2.58 °C, what is the enthalpy of this neutralization reaction (in kJ/mol)? Assume the density of the solution is 1.00g/mL and that the specific heat is...
QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below HX(aq)+ NaOH(aq) NaCN(aq)+ H20(1) Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH If the temperature of the calorimeter increases by 2.02 C, what is the enthalpy of this neutralization reaction (in kJ/mol)? Assume the density of the solution is 1.00g/mL and that the specific heat is 4.184 J/g "C...
The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 °C, and the final temperature after addition is 26.8 °c. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the...
Ferminow.com QUESTION 1 The weak acid, HX, is neutralized by sodium hydroxide as shown below: HX(aq) + NaOH(aq) NaCN(aq) + H2O(l). Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50,0 mL of 0.500 M NaOH. If the temperature of the calorimeter increases by 1.91 °C, what is the enthalpy of this neutralization reaction (in kJ/mol? Assume the density of the solution is 1.00g/mL and that the specific heat is...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH" (aq) - H20 (1) is -56.2...
help
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC. the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH(aq) → H20 (1) is -56.2...
i need help on the second page:
"calculate how many mols of HCL you used based on the volume
and molarity of the HCL"
and
"enthalpy of reaction" parts
Part B Heat of Reaction for HCl(aq) + NaOH (aq) NaCl (aq) + so H20 (1) Volume of 1.0 M HCl (ml) so 100 23.3 Volume of 1.0 M NaOH (ml) Mass of Solution (8) use 1.00 g/ml Ti solution (temp of HCl just before reaction) T solution (highest temp obtained)...
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