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Calculate the standard enthalpy change for the neutralization reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) when 50.0 mL of 1.0 M HCl reacts with 50.0 mL of 1.0 M NaOH in a constant pressure calorimeter. Assume the density of the final solution is the same as that of pure water (1 g/mL) and that the specific heat capacity of the final solution is 4.18 J/g K.
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Feb 3
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Chemical thermodynamics
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TroyPurton77
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1
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41
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid and sodium hydroxide, given the balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) and the enthalpy change of formation values: ∆Hf°(NaCl(aq)) = -407.3 kJ/mol ∆Hf°(H2O(l)) = -285.83 kJ/mol ∆Hf°(HCl(aq)) = -167.2 kJ/mol ∆Hf°(NaOH(aq)) = -469.11 kJ/mol
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Feb 3
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Chemical thermodynamics
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MireyaFlaher
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given the balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l). The enthalpies of formation for NaCl(aq) and H2O(l) are -407.3 kJ/mol and -285.8 kJ/mol, respectively. The specific heat capacity of the solution is 4.18 J/(g*K), and the mass of the resulting solution is 100 g.
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Feb 3
in
Chemical thermodynamics
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KristiMoore
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1
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73
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given the appropriate thermochemical equations and the following information:- Heat evolved during the reaction, Q = -58.35 kJ/mol- Moles of HCl used, n(HCl) = 0.05 mol- Concentration of NaOH solution, c(NaOH) = 2 M- Volume of NaOH solution used, V(NaOH) = 25.0 mL (assuming density of 1.00 g/mL)Show your calculations and include units in your final answer.
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Feb 3
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Chemical thermodynamics
by
DominickPlum
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1
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59
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given that the reaction produces water and sodium chloride as products. The molar enthalpy of formation for water is -285.8 kJ/mol and for NaCl is -411.2 kJ/mol. The balanced chemical equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
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Feb 3
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Chemical thermodynamics
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SilviaTorpy5
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) using the following information:- The standard enthalpy of formation for HCl is -92.31 kJ/mol - The standard enthalpy of formation for NaOH is -469.11 kJ/mol The balanced equation for the reaction is:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
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Feb 3
in
Chemical thermodynamics
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Lavonda96B02
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41
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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) in aqueous solutions. The balanced chemical equation for the reaction is as follows:HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) Given the enthalpy of formation for HCl(aq) is -167.2 kJ/mol, NaOH(aq) is -469.14 kJ/mol, NaCl(aq) is -407.3 kJ/mol, and H2O(l) is -285.83 kJ/mol. The reaction is carried out at standard temperature and pressure.
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Feb 3
in
Chemical thermodynamics
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ErickAshton2
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54
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Calculate the standard enthalpy change for the neutralization reaction between 50.0 mL of 0.100 M hydrochloric acid and 75.0 mL of 0.080 M sodium hydroxide. Given: the specific heat capacity of the solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. The balanced chemical equation for the reaction is HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l).
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Feb 3
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Chemical thermodynamics
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PearlEaston
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Calculate the standard enthalpy change for the neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH) in aqueous solution when 50.0 mL of 0.100 M HCl was used and 75.0 mL of 0.075 M NaOH was added. Assume that the specific heat capacity of the solution is 4.18 J/g·K and the density of the solution is 1.00 g/mL.
asked
Feb 3
in
Chemical thermodynamics
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LeeAlder0448
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0
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1
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29
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Calculate the standard enthalpy change for the neutralization of HCl with NaOH, given that the heat of formation of water is -285.8 kJ/mol, the heat of formation of NaCl is -411.1 kJ/mol, and the initial concentrations of HCl and NaOH are 1.0 M.
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Feb 3
in
Chemical thermodynamics
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WandaBalsill
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0
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1
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54
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Calculate the standard enthalpy change for the neutralization of 50.0 mL of 0.100 M hydrochloric acid with 50.0 mL of 0.100 M sodium hydroxide, assuming that the specific heat capacity of the resulting solution is 4.18 J/g °C and the density of the solution is 1.00 g/mL.
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Feb 3
in
Chemical thermodynamics
by
Melanie86K41
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1.7k
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0
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1
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61
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Calculate the standard enthalpy change for the neutralization of 50 mL of 0.1 M hydrochloric acid with 50 mL of 0.1 M sodium hydroxide at a constant temperature of 25°C, given that the specific heat capacity of the resulting solution is 4.18 J/g°C and its density is 1 g/mL.
asked
Feb 3
in
Chemical thermodynamics
by
WyattBriones
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1
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75
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Calculate the standard enthalpy change for the neutralization of 50 mL of 0.1 M hydrochloric acid with 50 mL of 0.1 M sodium hydroxide at a constant pressure and a temperature of 25°C. The balanced equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
asked
Feb 3
in
Chemical thermodynamics
by
AshleighFleg
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2.1k
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1
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49
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Calculate the standard enthalpy change for the neutralization of 25.0 mL of 1.0 M hydrochloric acid (HCl) with 25.0 mL of 1.0 M sodium hydroxide (NaOH) solution at 25°C, given that the specific heat capacity of the solutions is 4.18 J/g°C, and the density of the solutions is 1.00 g/mL.
asked
Feb 3
in
Chemical thermodynamics
by
LannyNewell
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1.8k
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0
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1
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71
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Calculate the standard enthalpy change for the neutralization of 25 mL of 0.10 M hydrochloric acid with 25 mL of 0.10 M sodium hydroxide. Assume the specific heat capacity of the solution to be 4.18 J/(g*K) and the density of the solution to be 1.00 g/mL. The temperature change observed during the reaction was 4.5°C.
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Feb 3
in
Chemical thermodynamics
by
GlenCaringto
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2.1k
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0
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1
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48
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Calculate the standard enthalpy change for the melting of 10 grams of ice at -10°C to liquid water at 20°C, given the specific heat capacity of water is 4.18 J/g°C and the enthalpy of fusion of water is 6.01 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
MarielScully
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1
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52
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Calculate the standard enthalpy change for the liquid-to-gas phase transition of water at 100°C and atmospheric pressure, given that the enthalpy of vaporization of water is 40.7 kJ/mol.
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Feb 3
in
Chemical thermodynamics
by
JoelPrentice
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1.4k
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0
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1
answer
74
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Calculate the standard enthalpy change for the given reaction using the given data:2H2(g) + O2(g) --> 2H2O(l)Given:ΔHf°(H2O(l)) = -285.83 kJ/molΔHf°(O2(g)) = 0 kJ/molΔHf°(H2(g)) = 0 kJ/mol
asked
Feb 3
in
Chemical thermodynamics
by
Denny08T6070
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2.5k
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0
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1
answer
61
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Calculate the standard enthalpy change for the fusion reaction of solid sodium chloride (NaCl) at 25°C, given the following information: ΔHf°[NaCl(s)] = -411 kJ/molΔHf°[Na(s)] = 108 kJ/molΔHf°[Cl2(g)] = 0 kJ/mol The balanced chemical equation for the fusion reaction of NaCl is:NaCl(s) → Na(s) + 1/2Cl2(g)
asked
Feb 3
in
Chemical thermodynamics
by
ErnestineScr
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1.6k
points)
0
votes
1
answer
83
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Calculate the standard enthalpy change for the fusion reaction of solid lithium at its melting point, assuming that the reaction is carried out under standard conditions.
asked
Feb 3
in
Chemical thermodynamics
by
UteKqe974841
(
1.9k
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