Question
In: Physics
In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M H2SO40.800 M H2SO4 was added...
In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M H2SO40.800 M H2SO4 was added to 50.0 mL50.0 mL of 0.370 M NaOH.0.370 M NaOH.
The reaction caused the temperature of the solution to rise from 23.40 ∘C23.40 ∘C to 25.92 ∘C.25.92 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184 J/(g⋅°C),4.184 J/(g⋅°C), respectively), what is Δ?ΔH for this reaction (per mole of H2OH2O produced)?
Assume that the total volume is the sum of the individual volumes.
Δ?=______ kj/mol H20
Consider these reactions, where M represents a generic metal.
-
2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)Δ?1=−889.0 kJ2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−889.0 kJ
-
HCl(g)⟶HCl(aq) Δ?2=−74.8 kJHCl(g)⟶HCl(aq) ΔH2=−74.8 kJ
-
H2(g)+Cl2(g)⟶2HCl(g) Δ?3=−1845.0 kJH2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ
-
MCl3(s)⟶MCl3(aq) Δ?4=−142.0 kJMCl3(s)⟶MCl3(aq) ΔH4=−142.0 kJ
Use the given information to determine the enthalpy of the reaction
2M(s)+3Cl2(g)⟶2MCl3(s)2M(s)+3Cl2(g)⟶2MCl3(s)
Δ?=_______ kj
Solutions
genius_generous answered 1 year agoRelated Solutions
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In a constant-pressure calorimeter, 50.0 mL of 0.330 M Ba(OH)2
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Assume that the total volume is the sum of the individual volumes
and that the density and heat capacity are equal to that of
water.
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M
NaF, CaF2 precipitates, as
shown in the net ionic equation below. The initial temperature of
both solutions is 25.00°C. Assuming
that the reaction goes to completion, and that the resulting
solution has a mass of 100.00 g and a heat
capacity the same as water, calculate the final temperature of the
solution.
Ca2+(aq) + 2 F-(aq) → CaF2(s)
ΔH° = –11.5 kJ
When trying to...
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M
NaF, CaF2 precipitates, as shown in the net ionic equation below.
The initial temperature of both solutions is 30.00°C. Assuming that
the reaction goes to completion, and that the resulting solution
has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C),
calculate the final temperature of the solution.
Ca2+(aq) + 2 F-(aq) →
CaF2(s) ΔH° = -11.5 kJ
30.55°C...
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...
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was added to 60.0 mL of 0.660 M HCl. The reaction caused the
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(per mole of H2O produced)? Assume that the total volume is the sum
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(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.
In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH)2 was added to 70.0 mL of...
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the solution has the same density and specific heat as water (1.00
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