Question

A 96.2 mL sample of 1.00 M NaOH is mixed with 48.1 mL of 1.00 M
H_{2}SO_{4} in a large Styrofoam coffee cup; the
cup is fitted with a lid through which passes a calibrated
thermometer. The temperature of each solution before mixing is
22.25 °C. After adding the NaOH solution to the coffee cup and
stirring the mixed solutions with the thermometer, the maximum
temperature measured is 30.90 °C. Assume that the density of the
mixed solutions is 1.00 g/mL, that the specific heat of the mixed
solutions is 4.18 J/(g·°C), and that no heat is lost to the
surroundings.

1. Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation.

2.Is any NaOH or H_{2}SO_{4} left in the
Styrofoam cup when the reaction is over? (Y or N)

3. Calculate the enthalpy change per mole of
H_{2}SO_{4} in the reaction. (kJ/mol)

Answer #1

A 90.2 mL sample of 1.00 M NaOH is mixed with 45.1 mL of 1.00 M
H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid
through which passes a calibrated thermometer. The temperature of
each solution before mixing is 21.45 °C. After adding the NaOH
solution to the coffee cup and stirring the mixed solutions with
the thermometer, the maximum temperature measured is 30.90 °C.
Assume that the density of the mixed solutions is 1.00...

A 90.2 mL sample of 1.00 M NaOH is mixed with 45.1 mL of 1.00 M
H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid
through which passes a calibrated thermometer. The temperature of
each solution before mixing is 21.05 °C. After adding the NaOH
solution to the coffee cup and stirring the mixed solutions with
the thermometer, the maximum temperature measured is 32.10 °C.
Assume that the density of the mixed solutions is 1.00...

A 97.2 mL sample of 1.00 M NaOH is mixed with 48.6 mL of 1.00 M
H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid
through which passes a calibrated thermometer. The temperature of
each solution before mixing is 23.05 °C. After adding the NaOH
solution to the coffee cup and stirring the mixed solutions with
the thermometer, the maximum temperature measured is 32.50 °C.
Assume that the density of the mixed solutions is 1.00...

A 100.0 ml sample of 1.00 M NaOH is mixed with 50.0 ml of 1.00 M
H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid
through which passes a calibrated thermometer. the temperature of
each solution before mixing is 22.5°C. After adding the NaOH
solution to the coffee cup and stirring the mixed solutions with
thermometer; the maximum temperature measured is 32.1 C. Assume
that the density of the mixed solutions is 1.00 g/ml that...

A 107.2 mL sample of 1.00 M NaOH is mixed with 53.6 mL of 1.00 M
H2SO4 in a large Styrofoam coffee cup; the
cup is fitted with a lid through which passes a calibrated
thermometer. The temperature of each solution before mixing is
22.45 °C. After adding the NaOH solution to the coffee cup and
stirring the mixed solutions with the thermometer, the maximum
temperature measured is 32.10 °C. Assume that the density of the
mixed solutions is 1.00...

A 100 mL sample of 0.300 M NaOH is mixed with a 100 mL sample of
0.300 M HNO3 in a coffee cup calorimeter. The two substances react
according to the following chemical equation: NaOH(aq) + HNO3(aq) →
NaNO3(aq) + H2O(l) Both solutions were initially at 35.0 °C. The
temperature of the solution after reaction was 37.0 °C. Estimate
the ΔHrxn (in kJ/mol NaOH). Assume: i) no heat is lost to the
calorimeter or the surroundings; and ii) the density...

A 50.0 mL sample of 0.300 M NaOH is mixed with a 50.0 mL sample
of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were
initially at 35.00°C and the temperature of the resulting solution
was recorded as 37.00°C, determine the ΔH°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 and the heat...

100.0 mL of 0.800 M aqueous NaOH and 50.00 mL of 0.800 M aqueous
H2SO4, each at 24.0°C, were mixed, see
equation:
2NaOH(aq) + H2SO4(aq) →
Na2SO4(aq) + 2H2O(l)
The final temperature achieved by the solution was 29.3 °C. Neglect
the heat capacity of the cup and the thermometer, and assume that
the solution of products has a density of exactly 1.00 g/mL and a
specific heat capacity of 4.18
J/(g•K). How much heat was absorbed by
the water?

10. In an effort to calculate the heat of neutralization of an
acid, a student mixed 50.0 mL of 1.0 M H2SO4 with 100 mL of 1.0 M
NaOH in a calorimeter and observes the temperature change. Write
the balanced chemical equation for this reaction.
If the initial temperature of the acid and base was 20.1 °C and
the temperature rose to 23.7 °C after mixing the two, what is the
heat of neutralization for H2SO4?
Assume that the solutions...

1)
A student reacts 25.0 mL of 0.225 M NaOH with 25.0 mL of 0.147 M
H2SO4. Write a balanced chemical equation to show this reaction.
Calculate the concentrations of NaOH and H2SO4 that remain in
solution, as well as the concentration of the salt that is formed
during the reaction.
2)
A student reacts 45.0 mL of 0.198 M Ba(OH)2 with 50.0 mL of
0.102 M H3PO4. Write a balanced chemical equation to show this
reaction. Note that the...

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