Question

When 30.5 mL of 0.515 M H2SO4 is added to 30.5 mL of 1.03 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/g×K.)

Answer #1

When 27.7 mL of 0.500 M H2SO4 is added to 27.7 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50°C, the temperature rises to
30.17°C. Calculate ?H of this reaction. (Assume that the total
volume is the sum of the individual volumes and that the density
and specific heat capacity of the solution are the same as for pure
water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)

When 26.6 mL of 0.500 M
H2SO4
is added to 26.6 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50
°
C, the temperature rises to 30.17
°
C. Calculate
Δ
H of this reaction. (Assume that the total
volume is the sum of the individual volumes and that the density
and specific heat capacity of the solution are the same as for pure
water.) (d for water = 1.00
g/mL;
c for water = 4.184 J/g
·...

When 23.8 mL of 0.500 M H2SO4 is added to 23.8 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50°C, the temperature rises to
30.17°C. Calculate ΔH of this reaction. (Assume that the total
volume is the sum of the individual volumes and that the density
and specific heat capacity of the solution are the same as for pure
water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)
?: kJ/mol H2O

When 26.5 mL of 0.500 M
H2SO4 is added to 26.5 mL of 1.00 M
KOH in a coffee-cup calorimeter at 23.50° C, the temperature rises
to 30.17° C. Calculate ΔH of this reaction. (Assume that
the total volume is the sum of the individual volumes and that the
density and specific heat capacity of the solution are the same as
for pure water.) (d for water = 1.00 g/mL; c for
water = 4.184 J/g°C).
Answer in kJ/molH2O

Enter your answer in the provided box.
When 22.9 mL of 0.500 M H2SO4 is
added to 22.9 mL of 1.00 M KOH in a coffee-cup calorimeter
at 23.50°C, the temperature rises to 30.17 °C. Calculate
ΔH of this reaction. (Assume that the total volume is the
sum of the individual volumes and that the density and specific
heat capacity of the solution are the same as for pure water.)
(d for water = 1.00 g/mL; c for water =...

In a constant-pressure calorimeter, 50.0 mL of 0.930 M H2SO4 was
added to 50.0 mL of 0.290 M NaOH. The reaction caused the
temperature of the solution to rise from 21.88 °C to 23.86 °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.

In a constant-pressure calorimeter, 55.0 mL of 0.840 M H2SO4 was
added to 55.0 mL of 0.260 M NaOH. The reaction caused the
temperature of the solution to rise from 21.91 °C to 23.68 °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.

In a constant-pressure calorimeter, 75.0 mL of 0.810 M H2SO4 was
added to 75.0 mL of 0.480 M NaOH. The reaction caused the
temperature of the solution to rise from 24.47 °C to 27.74 °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.

In a constant-pressure calorimeter, 60.0 mL of 0.780 M H2SO4 was
added to 60.0 mL of 0.490 M NaOH. The reaction caused the
temperature of the solution to rise from 23.53 °C to 26.87 °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.

In a constant-pressure calorimeter, 65.0 mL of 0.830 M H2SO4 was
added to 65.0 mL of 0.270 M NaOH. The reaction caused the
temperature of the solution to rise from 21.71 °C to 23.55 °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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