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D Question 5 2 pts Suppose 160 mL of 8.0 M NaOH(aq) is added to 167...
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I already asked this question, BUT I still NEED help.
Please! No one has answered it!
Suppose 160 mL of 8.0 M NaOH(aq) is added to 197 mL of 6.0 M HNO3(aq) to make a solution with a density of 1.1 g/mL and a specific heat of 4.1 J/gxK. If the initial temperature of both solutions is 295 K, what will be the final temperature (K)? Enter your answer as an integer. H+(aq) + OH-(aq) → H2O() ΔHo=-55.8 kJ/mol
Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 ...
PART ONE:
PART TWO:
PART THREE:
PART FOUR:
Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...
C) 3400 D ) 2000 Q10: 1.0 L of 1 M NaOH(aq) and 1.0 L of...
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...
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...
Mixing 25.0 mL of 1.2 M HCland 25.0 mL of 1.1 M NaOH were mixed. The...
Mixing 25.0 mL of 1.2 M HCland 25.0 mL of 1.1 M NaOH were mixed. The temperature of the initial solution was 22.4 oC. Assuming a Heat of Neutralization of -55.8 KJ/mol, what would the final temperature be if the specific heat for this solution is 4.03 J/g?
solve the blanks Data and Calculations 1. AH (neutralization & dilution) of 10 M H:SO4 and 1.00 M NaOH Keain...
solve the blanks
Data and Calculations 1. AH (neutralization & dilution) of 10 M H:SO4 and 1.00 M NaOH Keain Data Trial 1 Trial 2 Initial temperature of 10 M H2SO (5.0 mL in a graduated eylinder) 23.2 23.8 C C Initial temperature of calorimeter (50.0 mL of 1.00 M NaOH 45.0 mL water) 22.8 °C 2 1.5 °C Final temperature of the mixed solutions in calorimeter (50 mL 1.00 M NaOH 45.0 mL water 5.0 mlL 10 M H2SO)...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.0°C and the temperature of the resulting solution was recorded as 37.0°C, determine the DH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2)that the density(1.00 g/mL) and the specific...
Data and Results: Part A M (HCI): Volume HCl(aq): Reaction 2: Heat of Neutralization M(NaOH) 50.0...
Data and Results: Part A M (HCI): Volume HCl(aq): Reaction 2: Heat of Neutralization M(NaOH) 50.0 mL (+0.5 mL) Volume NaOH(aq): 20, 9 °C Final Temperature: 6.7 (not from the data above) 1.0 50-0 ML (+0.5 mL) 27.6 °C Initial Temperature: AT (from plot) Mass of Solution: (show all calculations) Moles H*:(show all calculations) Moles OH :(show all calculations) 0.05 moles H 0.05 moles OH AH experimental: (show all calculations) kJ/mol AH (theoretical): (see page 8) (show all calculations) kJ/mol...
When 60.0 mL of a 0.400 M solution of HNO3 (aq) is combined with 60.0 mL...
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....
In a constant-pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of...
In a constant-pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of 0.620 M HCI. The reaction caused the temperature of the solution to rise from 24.11 °C to 28.33 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 Jlg. °C, respectively), what is AH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/mol H,o
I already asked this question, BUT I still NEED help.
Please! No one has answered it!
Suppose 160 mL of 8.0 M NaOH(aq) is added to 197 mL of 6.0 M HNO3(aq) to make a solution with a density of 1.1 g/mL and a specific heat of 4.1 J/gxK. If the initial temperature of both solutions is 295 K, what will be the final temperature (K)? Enter your answer as an integer. H+(aq) + OH-(aq) → H2O() ΔHo=-55.8 kJ/mol
PART ONE:
PART TWO:
PART THREE:
PART FOUR:
Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...
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)...
solve the blanks
Data and Calculations 1. AH (neutralization & dilution) of 10 M H:SO4 and 1.00 M NaOH Keain Data Trial 1 Trial 2 Initial temperature of 10 M H2SO (5.0 mL in a graduated eylinder) 23.2 23.8 C C Initial temperature of calorimeter (50.0 mL of 1.00 M NaOH 45.0 mL water) 22.8 °C 2 1.5 °C Final temperature of the mixed solutions in calorimeter (50 mL 1.00 M NaOH 45.0 mL water 5.0 mlL 10 M H2SO)...
Data and Results: Part A M (HCI): Volume HCl(aq): Reaction 2: Heat of Neutralization M(NaOH) 50.0 mL (+0.5 mL) Volume NaOH(aq): 20, 9 °C Final Temperature: 6.7 (not from the data above) 1.0 50-0 ML (+0.5 mL) 27.6 °C Initial Temperature: AT (from plot) Mass of Solution: (show all calculations) Moles H*:(show all calculations) Moles OH :(show all calculations) 0.05 moles H 0.05 moles OH AH experimental: (show all calculations) kJ/mol AH (theoretical): (see page 8) (show all calculations) kJ/mol...
In a constant-pressure calorimeter, 60.0 mL of 0.310 M Ba(OH)2 was added to 60.0 mL of 0.620 M HCI. The reaction caused the temperature of the solution to rise from 24.11 °C to 28.33 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 Jlg. °C, respectively), what is AH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/mol H,o
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