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A constant-volume calorimeter was calibrated by carrying out a reaction known to release 1.15 kJ of...
please show steps =-72-88 kJ/mol. 10. A reaction known to release 1.78kJ of heat takes place in a calorimeter contai...
please show steps
=-72-88 kJ/mol. 10. A reaction known to release 1.78kJ of heat takes place in a calorimeter containing 0.100L of solution and the temperature rose by 3.65°C. The calorimeter was then rinsed out and emptied. To the empty calorimeter was placed a small piece of calcium carbonate and 0.100L of dilute HCI was poured over it in the same calorimeter). The temperature of the calorimeter then rose by 3.57°C. What is the heat, q, in kJ released by...
In one of the General Chemistry experiments, you used a coffee-cup calorimeter to measure the heat...
In one of the General Chemistry experiments, you used a coffee-cup calorimeter to measure the heat of neutralization of selected acid-base reactions. The calorimeter consisted of two nested Styrofoam cups with a cardboard lid. A temperature probe was lowered in the solution through a hole in the lid. Is a coffee-cup calorimeter a constant-volume or a constant-pressure device? Is a coffee-cup calorimeter adiabatic? The coffee-cup calorimeter was calibrated by using the neutralization reaction between sodium hydroxide and hydrochloric acid. The...
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00...
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00 M hydrochloric acid with 100 mL of 1.20 M sodium hydroxide. The initial temperature was 22.88 °C and the final temperature was 29.39 °C. Calculate the calorimeter constant for the reaction. HCl (aq) + NaOH (aq) NaCl (aq) + H2O (∆H°rxn = -58.3 kJ/mol) 2. The same calorimeter was used for the dissolution of 8.86 g sample of lithium chloride in 100.0 mL of...
2. Consider the reaction of 50.0 mL of 1.15 M HC2H302 with 50.0 mL of 1.30...
2. Consider the reaction of 50.0 mL of 1.15 M HC2H302 with 50.0 mL of 1.30 M NH3. a. Give the net ionic reaction between these two reagents. H+(99) + NH3(aq) →NH4+(29) b. Calculate the moles of each reactant and indicate which reactant is the limiting reagent. Moles of HC2H2O2: 0.058 moles Moles of NH3: 0.065 moles c. Once the two reactant solutions are brought to the same initial temperature, they are mixed in a calorimeter, also at the same...
Part 2, find AH°rxn =kJ/mol Two solutions are mixed in a coffee cup calorimeter both are...
Part 2, find AH°rxn =kJ/mol Two solutions are mixed in a coffee cup calorimeter both are initially at 22.60°C. When a 100.0 mL volume of 1.00 M AgNO3 solution is mixed with a 100.0 mL sample of 0.500 M NaCl solution, the temperature in the calorimeter rises to 28.30°C (assume no heat is lost to the surroundings and the density and heat capacity of the solutions is the same as that of water). Determine the AHºrxn for the reaction as...
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH)2 was added to 55.0 mL of...
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH)2 was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 22.52 °C to 27.3 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g. °C,) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,...
In a constant-pressure calorimeter, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of...
In a constant-pressure calorimeter, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 24.49 C to 29.26 C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g• C) respectively), what is ?H for this reaction (per mole H2O produced)? Assume and the total volume is the sum of the individual volumes. ?H= _______ kJ/mol H2O
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in an unknown...
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in an unknown volume of water (where X is a hypothetical metal) X 2 H20X(OH)2 + H2 In this process, the water temperature rose from 25.0 °C to 36.7 °C. If 0.00814 mol of "X" was consumed during the reaction, and the AH of this reaction with respect to the system is -1447 kJ mol-1 , what volume of water (in mL) was present in the calorimeter?...
6. (30 points) Given reaction: Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2H20(0) AH = ....
6. (30 points) Given reaction: Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2H20(0) AH = . 118 kJ A student mixed 200.0 mL of 0.200 M HCl with 350.0 mL of 0.200 M Ba(OH)2 in a coffee cup calorimeter at 25.0°C (The initial temperatures of both solutions and the cup were 25.0°C). The heat capacity of the imeter is 58.3J/°C. Assume the density and the specific heat capacity of the mixed solution are the same water (d=1.00 g/mL, Cs =...
< Question 11 of 14 > In a constant-pressure calorimeter, 75.0 mL of 0.920 M H2SO4...
< Question 11 of 14 > In a constant-pressure calorimeter, 75.0 mL of 0.920 M H2SO4 was added to 75.0 mL of 0.300 M NaOH. The reaction caused the temperature of the solution to rise from 21.12 °C to 23.16 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/(g · °C), respectively), what is AH for this reaction (per mole of H0 produced)? Assume that the total volume is the sum...
please show steps
=-72-88 kJ/mol. 10. A reaction known to release 1.78kJ of heat takes place in a calorimeter containing 0.100L of solution and the temperature rose by 3.65°C. The calorimeter was then rinsed out and emptied. To the empty calorimeter was placed a small piece of calcium carbonate and 0.100L of dilute HCI was poured over it in the same calorimeter). The temperature of the calorimeter then rose by 3.57°C. What is the heat, q, in kJ released by...
2. Consider the reaction of 50.0 mL of 1.15 M HC2H302 with 50.0 mL of 1.30 M NH3. a. Give the net ionic reaction between these two reagents. H+(99) + NH3(aq) →NH4+(29) b. Calculate the moles of each reactant and indicate which reactant is the limiting reagent. Moles of HC2H2O2: 0.058 moles Moles of NH3: 0.065 moles c. Once the two reactant solutions are brought to the same initial temperature, they are mixed in a calorimeter, also at the same...
Part 2, find AH°rxn =kJ/mol Two solutions are mixed in a coffee cup calorimeter both are initially at 22.60°C. When a 100.0 mL volume of 1.00 M AgNO3 solution is mixed with a 100.0 mL sample of 0.500 M NaCl solution, the temperature in the calorimeter rises to 28.30°C (assume no heat is lost to the surroundings and the density and heat capacity of the solutions is the same as that of water). Determine the AHºrxn for the reaction as...
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH)2 was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 22.52 °C to 27.3 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g. °C,) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,...
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in an unknown volume of water (where X is a hypothetical metal) X 2 H20X(OH)2 + H2 In this process, the water temperature rose from 25.0 °C to 36.7 °C. If 0.00814 mol of "X" was consumed during the reaction, and the AH of this reaction with respect to the system is -1447 kJ mol-1 , what volume of water (in mL) was present in the calorimeter?...
6. (30 points) Given reaction: Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2H20(0) AH = . 118 kJ A student mixed 200.0 mL of 0.200 M HCl with 350.0 mL of 0.200 M Ba(OH)2 in a coffee cup calorimeter at 25.0°C (The initial temperatures of both solutions and the cup were 25.0°C). The heat capacity of the imeter is 58.3J/°C. Assume the density and the specific heat capacity of the mixed solution are the same water (d=1.00 g/mL, Cs =...
< Question 11 of 14 > In a constant-pressure calorimeter, 75.0 mL of 0.920 M H2SO4 was added to 75.0 mL of 0.300 M NaOH. The reaction caused the temperature of the solution to rise from 21.12 °C to 23.16 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/(g · °C), respectively), what is AH for this reaction (per mole of H0 produced)? Assume that the total volume is the sum...
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