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need help with trial 1
EQUATIONS and CALCULATIONS: 1) 2) 3) 4) 5) 6) 7) In...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s)...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s)...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
need the Hess law calculations please!!! Thanks 3% Trial 4 What is the concentration of the...
need the Hess law calculations please!!!
Thanks
3% Trial 4 What is the concentration of the stock H.O, solution? How much heat should be released when 10.0 mL of H., decompose? Your answer must be in units of kJ Trial Trial 2 Trial 3 Mass of H.Ozused (9) 0.055g 0.0589 0.052g Moles of H.O.decomposed (mol) 0.0016 0.0017 0.0015 Final Temperature (T) (°C) 38.00 138.4°C 13.1°C Initial temperature (T) ("C) 22:2°C 22.30 22.3°C Change in temperature: AT= T.-T (°C) 15.800 16.1°C...
I need help with 11 and 12 please. Data Table Mixture NaCl (s) + H2O (1)...
I need help with 11 and 12 please.
Data Table Mixture NaCl (s) + H2O (1) T (initial) T, (final) AT (T-T) -.20 25.00 24.80 NaNO, (s) + H2O (1) 24.99 24.11 -.88 NaCH,COO + H2O (1) 24.99 25.91 .82 Use your experimental data to answer the following questions: 7. Calculate AT (AT = T2-T) for each mixture and record the results in the data table. 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat...
please help When a solid dissolves in water, heat may be evolved or absorbed. The heat...
please help
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.85 g of CaCl2(s) are dissolved in 100.10 g of water, the temperature of the solution increases from 24.36 to 25.89 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer In the laboratory a general chemistry student finds that when 9.66 g of CSCI(S) are dissolved in 106.80 g of water, the temperature of the solution drops from 22.55 to 19.99 °C. Cardboard or Styrofoam lid The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate...
Use wie Nererences to access poi lallt values il leeueu IUI LIIS uuestivII. A student determines...
Use wie Nererences to access poi lallt values il leeueu IUI LIIS uuestivII. A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.63 g of CoSO4(s) is dissolved in 111.00 g of water, the temperature of the solution increases from 25.00 to 26.88 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH...
The In the laboratory a "coffee cup calorimeter, or constant pressure calorimeter, is frequently used to determi...
The In the laboratory a "coffee cup calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 61.44 grams of titanium to 97.72 °C and then drops it into a cup containing 83.69 grams of water at 21.75 °C. She measures the final temperature to be 27.96 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant)...
please help When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving)...
please help
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 1.61 g of CaCl(s) are dissolved in 109.50 g of water, the temperature of the solution increases from 25.78 to 28.44 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in...
i just need help on this first question, the others parts are just added information if...
i just need help on this first question, the others parts are
just added information if its needed
1. First, calculate the amount of heat energy, Ical, produced in each reaction using Eq. 1 from the Introduction. Convert Vwater to Mwater using a density value of 1.00 g/mL, and s = 4.18 J/(g•°C). Next, calculate the number of moles of NaNO3 (and NH4Cl) present in each reaction using Eq. 2. Finally, calculate the enthalpy change, AH, for each reaction in...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
need the Hess law calculations please!!!
Thanks
3% Trial 4 What is the concentration of the stock H.O, solution? How much heat should be released when 10.0 mL of H., decompose? Your answer must be in units of kJ Trial Trial 2 Trial 3 Mass of H.Ozused (9) 0.055g 0.0589 0.052g Moles of H.O.decomposed (mol) 0.0016 0.0017 0.0015 Final Temperature (T) (°C) 38.00 138.4°C 13.1°C Initial temperature (T) ("C) 22:2°C 22.30 22.3°C Change in temperature: AT= T.-T (°C) 15.800 16.1°C...
I need help with 11 and 12 please.
Data Table Mixture NaCl (s) + H2O (1) T (initial) T, (final) AT (T-T) -.20 25.00 24.80 NaNO, (s) + H2O (1) 24.99 24.11 -.88 NaCH,COO + H2O (1) 24.99 25.91 .82 Use your experimental data to answer the following questions: 7. Calculate AT (AT = T2-T) for each mixture and record the results in the data table. 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat...
please help
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.85 g of CaCl2(s) are dissolved in 100.10 g of water, the temperature of the solution increases from 24.36 to 25.89 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer In the laboratory a general chemistry student finds that when 9.66 g of CSCI(S) are dissolved in 106.80 g of water, the temperature of the solution drops from 22.55 to 19.99 °C. Cardboard or Styrofoam lid The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate...
Use wie Nererences to access poi lallt values il leeueu IUI LIIS uuestivII. A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.63 g of CoSO4(s) is dissolved in 111.00 g of water, the temperature of the solution increases from 25.00 to 26.88 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH...
The In the laboratory a "coffee cup calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 61.44 grams of titanium to 97.72 °C and then drops it into a cup containing 83.69 grams of water at 21.75 °C. She measures the final temperature to be 27.96 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant)...
please help
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 1.61 g of CaCl(s) are dissolved in 109.50 g of water, the temperature of the solution increases from 25.78 to 28.44 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in...
i just need help on this first question, the others parts are
just added information if its needed
1. First, calculate the amount of heat energy, Ical, produced in each reaction using Eq. 1 from the Introduction. Convert Vwater to Mwater using a density value of 1.00 g/mL, and s = 4.18 J/(g•°C). Next, calculate the number of moles of NaNO3 (and NH4Cl) present in each reaction using Eq. 2. Finally, calculate the enthalpy change, AH, for each reaction in...
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