Heats of Reaction – Hess’ LawName _______________________________In this experiment you will determine and compare the quantity of heat energy released in three exothermic chemical reactions.Reaction 1: Solid sodium hydroxide dissolves in water to form an aqueous solution of ions.NaOH(s) → Na+(aq) + OH-(aq) + x1 kJReaction 2: Solid sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride.NaOH(s) + H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x2 kJReaction 3: An aqueous solution of sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride.Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x3 kJIn order to accurately measure the heat released in each reaction, we will be using a calorimeter. (For this experiment a styrofoam cup will act as the calorimeter). The change in temperature that occurs for each reaction will be used to calculate the energy released in kilojoules per mole of sodium hydroxide used. We can assume for our calculations that any heat transferred to the styrofoam and surrounding air will be negligible. We can also assume that the specific heat of water is 4.18 J/g°C.

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19-12-2022
Chemistry

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Heats of Reaction – Hess’ LawName _______________________________In this experiment you will determine and compare the quantity of heat energy released in three exothermic chemical reactions.Reaction 1: Solid sodium hydroxide dissolves in water to form an aqueous solution of ions.NaOH(s) → Na+(aq) + OH-(aq) + x1 kJReaction 2: Solid sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride.NaOH(s) + H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x2 kJReaction 3: An aqueous solution of sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride.Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x3 kJIn order to accurately measure the heat released in each reaction, we will be using a calorimeter. (For this experiment a styrofoam cup will act as the calorimeter). The change in temperature that occurs for each reaction will be used to calculate the energy released in kilojoules per mole of sodium hydroxide used. We can assume for our calculations that any heat transferred to the styrofoam and surrounding air will be negligible. We can also assume that the specific heat of water is 4.18 J/g°C.

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aamirmajeed5100 aamirmajeed5100 · Answer 1 · 2022-12-24T07:02:31-05:00

This data can then be used to confirm or disprove Hess’s law.

The first step in this experiment is to measure the mass of sodium hydroxide and water needed for each reaction. This should be done using a mass balance or digital scale.

After the masses have been determined, the sodium hydroxide and water should be added to the styrofoam cup in the correct proportions so that they can react. The temperature of the water should be recorded before the reaction occurs. Once the reaction has taken place, the temperature of the water should be recorded again.

Using the data collected in the experiment, the heat of the reaction for each of the three reactions can be calculated. For reaction 1, the heat of the reaction can be calculated using the formula q = m*C*∆T, where m is the mass of water, C is the specific heat capacity of water, and ∆T is the change in temperature. For reactions 2 and 3, the heat of the reaction can be calculated using the equation q = m*x*∆T, where m is the mass of sodium hydroxide, x is the number of moles of sodium hydroxide, and ∆T is the change in temperature.

Once the heat of the reaction has been calculated, it can be compared to determine which reaction releases the most energy. This data can then be used to confirm or disprove Hess’s law.

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