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A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL...
a) A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL...
a) A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 18.1 oC before mixing and 39.1 oC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔH for the process: CuSO4(1M)+ 2KOH(2M) →Cu(OH)2(s) + K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the...
A 50.0-ml sample of a 1.00 m solution of cuso4 is mixed with 50.0 ml of...
A 50.0-ml sample of a 1.00 m solution of cuso4 is mixed with 50.0 ml of 2.00 M KOH in a calorimeter. the temperature of both solutions was 20.2C before mixing and 26.3C after mixing. The heat capacity of the calorimeter is 12.1 J/k. from these data calculate ΔH for the process: CuSO4 (1M) +2KOH (2M)---->Cu(OH)2 (s) + K2SO4 (0.5M) Assume the specific heat and density of the solution after mixing are the same as those of pure water and...
A 50 ml sample of a 1.0 M solution of CuSO4 is mixed with 50 mL...
A 50 ml sample of a 1.0 M solution of CuSO4 is mixed with 50 mL of 2.0 M KOH in a calorimeter. The temperature of both solutions was 23.9°C before mixing and 33.5°C ofter mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate AH for the process: CuSO4 (1M) + 2KOH (2M) - Cu(OH)2 (8) + K2504 (0.5M) Assume that the specific heat and density of the solution after mixing are the same as...
Part A before mong and 34C er mang. The best capacity of the A 50.0 mL...
Part A before mong and 34C er mang. The best capacity of the A 50.0 mL sample of a 100 M solution of C o m e with 50.0 mL of 200 M ROH in a calorimeterThe temperature of both solutions was 209" calorimeter is 121JX From these da culate H for the process CuSO (IM) + 2KOR (2) Cu(OH),(-) + K 80.(0.5M) Assume that the specific heat and density of the solution after wing are the same as those...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
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 v...
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...
Two solutions, 50.0 mL of 1.00 M BaCl2 (aq) and 50.0 mL of 1.00 M Na2SO4...
Two solutions, 50.0 mL of 1.00 M BaCl2 (aq) and 50.0 mL of 1.00 M Na2SO4 (aq), both at 21.5 ° C, are mixed in a thermometer. The heat capacity of the thermometer with the solutions in is 1.23 kJ / ° C. During mixing, the temperature of the solution rises to 23.4 ° C. How much heat (qrxn) is released from the reaction that occurs when 1 mole of BaSO4 (s) is precipitated? Give the answer in kJ.
In a constant-pressure calorimeter, 50.0 mL of 0.320 M Ba(OH), was added to 50.0 mL of 0.640 M HCI. The reaction ca...
In a constant-pressure calorimeter, 50.0 mL of 0.320 M Ba(OH), was added to 50.0 mL of 0.640 M HCI. The reaction caused the temperature of the solution to rise from 21.35 'C to 25.71 '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,0 produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0
In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of...
In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 22.91 °C to 27.54 °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.
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are...
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are told concentration of the NaOH solution you used was 5% less than indicated on its label and asked to recalculate your enthalpy of neutralization. Will the recalculated cment value be larger, smaller, or the same as you originally calculated? b. Now consider the HCl you used in your experiment, if the concentration was 5% higher than that stated on its label, what will be...
A 50 ml sample of a 1.0 M solution of CuSO4 is mixed with 50 mL of 2.0 M KOH in a calorimeter. The temperature of both solutions was 23.9°C before mixing and 33.5°C ofter mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate AH for the process: CuSO4 (1M) + 2KOH (2M) - Cu(OH)2 (8) + K2504 (0.5M) Assume that the specific heat and density of the solution after mixing are the same as...
Part A before mong and 34C er mang. The best capacity of the A 50.0 mL sample of a 100 M solution of C o m e with 50.0 mL of 200 M ROH in a calorimeterThe temperature of both solutions was 209" calorimeter is 121JX From these da culate H for the process CuSO (IM) + 2KOR (2) Cu(OH),(-) + K 80.(0.5M) Assume that the specific heat and density of the solution after wing are the same as those...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
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...
In a constant-pressure calorimeter, 50.0 mL of 0.320 M Ba(OH), was added to 50.0 mL of 0.640 M HCI. The reaction caused the temperature of the solution to rise from 21.35 'C to 25.71 '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,0 produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0
In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 22.91 °C to 27.54 °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.
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are told concentration of the NaOH solution you used was 5% less than indicated on its label and asked to recalculate your enthalpy of neutralization. Will the recalculated cment value be larger, smaller, or the same as you originally calculated? b. Now consider the HCl you used in your experiment, if the concentration was 5% higher than that stated on its label, what will be...
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