Question
In: Chemistry
When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C...
When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C water, the final temperature was measured as 40.8 °C. Assume the density for water is 1.000 g/mL regardless of temperature.
a. Determine the magnitude of the heat lost by the hot water.
b. determine the magnitude of the heat gained by the room temperature water.
c. determine the heat gained by the calorimeter
d. determine the calorimeter constant.
Solutions
queen_honey_blossom answered 7 months agoRelated Solutions
A 50.0-g sample of liquid water at 25.0°C is mixed with 35.0 g of water at...
A 50.0-g sample of liquid water at 25.0°C is mixed with 35.0 g
of water at 89.0°C. The final temperature of the water is
________°C.
1a )When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of...
1a )When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of
0.500 M NaOH at 25.0°C in a coffee cup calorimeter, the temperature
of the mixture rises to 28.2°C. What is the enthalpy of reaction
per mole of acid? Assume the mixture has a specific heat capacity
of 4.18 J/(g ? K) and that the densities of the reactant solutions
are both 1.00 g/mL.
1b) Consider the following reaction: 2 PbS (s) + 3 O2...
50 ml of hot water was mixed with 50ml of cold water in a calorimeter. The...
50 ml of hot water was mixed with 50ml of cold water in a
calorimeter. The initial temperature of the cold water is
22°C, the initial temperautre of hot water is
79°C, the average temperature is
50.5°C, the temperature at time 0 is
46.333°C.
What is the heat lost by hot water, the heat gained by cold
water, the heat gained by calorimeter in J, temperature change of
the calorimeter, the heat capacity (C) of the calorimeter in
J/°C, and...
a. 0.130 g of HCl is in 35.0 mL of water. This is mixed with 50.0...
a. 0.130 g of HCl is in 35.0 mL of water. This is mixed with
50.0 mL of 0.185 M Sr(OH)2. What is the pH of the
resulting solution?
b. Calculate the pH of a solution prepared by mixing 125.0 mL of
0.0120 M HCl with 25.0 mL of 0.0420 M Ba(OH)2?
c.
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50...
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50
M NaOH solution at 25.2°C are reacted together to give a final
temperature of 44.1°C. The specific heat of the solution is 3.88
J/g°C and it weighs 76.6 grams. From this information,
determine:
a. the limiting reactant for this reaction
b. the heat produced by the reaction (q) in units of Joules.
c. the enthalpy of the reaction (∆H) in units of kJ/mole.
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of...
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2
was added to 60.0 mL of 0.660 M HCl. The reaction caused the
temperature of the solution to rise from 21.42 °C to 25.92 °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 ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of...
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2
was added to 60.0 mL of 0.660 M HCl. The reaction caused the
temperature of the solution to rise from 21.67 °C to 26.17 °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 ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
In a constant-pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of...
In a constant-pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2
was added to 60.0 mL of 0.640 M HCl. The reaction caused the
temperature of the solution to rise from 23.05 °C to 27.41 °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 ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
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 HCl. The reaction caused the
temperature of the solution to rise from 22.61 °C to 26.83 °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 ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of...
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2
was added to 60.0 mL of 0.660 M HCl. The reaction caused the
temperature of the solution to rise from 23.72 °C to 28.22 °C. If
the solution has the same density and specific heat as water (1.00
g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
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