In a constant-pressure calorimeter, 65.0 mL of 0.300 M Ba(OH)2 was added to 65.0 mL of 0.600 M HCl.?
2016-02-29 7:18 pm
The reaction caused the temperature of the solution to rise from 22.35 °C to 26.44 °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.
回答 (1)
2016-02-29 7:30 pm
Ba(OH)₂ + 2HCl → BaCl₂ + 2H₂O
1 mole of Ba(OH)₂ reacts with 2 moles of HCl to give 2 moles of H₂O
Initial number of moles of Ba(OH)₂ = 0.300 × (65.0/1000) = 0.0195 mol
Initial number of moles of HCl = 0.600 × (65.0/1000) = 0.0390 mol
When all Ba(OH)₂, no. of moles of HCl needed = 0.0195 × 2 = 0.0390 mol
Both the reactants completely react.
Number of moles of water formed = 0.0390 × 1 = 0.0390 mol
Heat released = m c ΔT = (65 + 65) × 4.184 × (26.44 - 22.35) = 2225 J = 2.225 kJ
ΔH = -2.225/0.0390 = 57.1 kJ/mol of H₂O produced
1 mole of Ba(OH)₂ reacts with 2 moles of HCl to give 2 moles of H₂O
Initial number of moles of Ba(OH)₂ = 0.300 × (65.0/1000) = 0.0195 mol
Initial number of moles of HCl = 0.600 × (65.0/1000) = 0.0390 mol
When all Ba(OH)₂, no. of moles of HCl needed = 0.0195 × 2 = 0.0390 mol
Both the reactants completely react.
Number of moles of water formed = 0.0390 × 1 = 0.0390 mol
Heat released = m c ΔT = (65 + 65) × 4.184 × (26.44 - 22.35) = 2225 J = 2.225 kJ
ΔH = -2.225/0.0390 = 57.1 kJ/mol of H₂O produced
收錄日期: 2021-04-18 14:31:19
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20160229111802AABuJoX