In a constant-pressure calorimeter, 65.0 mL of 0.800 M H2SO4 was added to 65.0 mL of 0.310 M NaOH. The reaction caused the temperature of the solution to rise from 21.61 °C to 23.72 °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.
what is the delta H of the reaction in kJ/mol of H2O?
In a constant-pressure calorimeter, 65.0 mL of 0.800 M H2SO4 was added to 65.0 mL of...
In a constant-pressure calorimeter, 65.0 mL of 0.810 M H2SO4 was added to 65.0 mL of 0.250 M NaOH. The reaction caused the temperature of the solution to rise from 24.29 °C to 25.99 °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 0.760 M H2SO4 was added to 65.0 mL of 0.370 M NaOH . The reaction caused the temperature of the solution to rise from 21.62 ∘ C to 24.14 ∘ 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 Δ H for this reaction (per mole of H 2 O produced)? Assume that...
In a constant-pressure calorimeter, 65.0 mL of 0.320 M Ba(OH)2 was added to 65.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 21.34 °C to 25.70 °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.
n a constant‑pressure calorimeter, 65.0 mL of 0.310 M Ba(OH)2 was added to 65.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 23.58 ∘C to 27.80 ∘C. If the solution has the same density and specific heat as water ( 1.00 g/mL and 4.184J/g⋅K,) respectively), what is Δ? for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes.
Please show all work In a constant-pressure calorimeter, 65.0 mL of 0.820 M H,SO, was added to 65.0 mL of 0.430 M NaOH. The reaction caused the temperature of the solution to rise from 23.87°C 10 26.80 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/(.c), respectively), what is AH for this reaction (per mole of H, produced)? Assume that the total volume is the sum of the individual volumes. AH...
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 HCI. The reaction caused the temperature of the solution to rise from 24.11 °C to 28.33 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 Jlg. °C, respectively), what is AH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/mol H,o
In a constant pressure calorimeter 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL of 0.620 M HCl. the reactions caused the temperature of the solution to rise from 23.77 c to 27.99 c if the solution has the same density and same specific heat as water (1.00 g/mL and 4.184 j/g c ) what is triangle H 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, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 24.49 C to 29.26 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 ?H for this reaction (per mole H2O produced)? Assume and the total volume is the sum of the individual volumes. ?H= _______ kJ/mol H2O
In a constant-pressure calorimeter, 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL of 0.620 M HCI The reaction caused the temperature of the solution to rise from 23.56 ? to 27.78 ?, what is ?? for this reaction (KJ released per mole of H2O produced)? 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 Number kJ/ mol H,O
In a constant-pressure calorimeter, 55.0 mL of 0.310 M Ba(OH), was added to 55.0 mL of 0.620 M HCI. The reaction caused the temperature of the solution to rise from 22.30 °C to 26.52 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g. 'C) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0