Recent questions in ThermoChemistry

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1 answer 71 views

A student needs to find out how much heat is released or absorbed when 100 mL of 0.1 mol/L solution of barium chloride (BaCl2) is mixed with 150 mL of 0.1 mol/L solution of sodium sulfate (Na2SO4) at 25°C. Given the enthalpy of precipitation of BaSO4 as -256 kJ/mol, calculate the enthalpy change (in kJ) for the reaction that occurs and determine whether the reaction is exothermic or endothermic.

asked Jan 22 in ThermoChemistry by JaunitaSchur (410 points)

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1 answer 62 views

A student needs to determine the enthalpy change (ΔH) for the reaction between ammonium nitrate (NH4NO3) and water (H2O) using Hess's Law calculations. Given the following information: - ΔHf° (NH4NO3) = -365.4 kJ/mol- ΔHf° (HNO3) = -207.3 kJ/mol- ΔHf° (NH4+) = -132.5 kJ/mol- ΔHf° (NO3-) = -206.1 kJ/mol- ΔHf° (H2O) = -285.83 kJ/molFormulate the thermochemical equation for the reaction by using the given data and Hess's Law calculations, and then calculate the enthalpy change for the reaction.

asked Jan 22 in ThermoChemistry by Addie5174877 (710 points)

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1 answer 81 views

A student needs to calculate the standard enthalpy of formation of magnesium oxide, MgO, using Hess's Law. The student has access to the following reactions and their corresponding enthalpy changes:1. Mg(s) + 1/2O2(g) → MgO(s) ΔH = -601.8 kJ/mol2. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH = -450.7 kJ/mol3. H2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ/molWhat is the standard enthalpy of formation of MgO from its elements?

asked Jan 22 in ThermoChemistry by BrittneyN44 (350 points)

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1 answer 39 views

A student needs to calculate the standard enthalpy change of combustion for propane using Hess's Law. They have the following information: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH° = -2220 kJ/mol 2H2(g) + O2(g) → 2H2O(l) ΔH° = -484 kJ/mol 3C(s) + 2H2(g) → C3H8(g) ΔH° = +51 kJ/mol What is the standard enthalpy change of combustion for propane?

asked Jan 22 in ThermoChemistry by DarcyStevens (510 points)

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1 answer 44 views

A student needs to calculate the heat of mixing for a 50 mL solution containing 0.1 M HCl and 0.1 M NaOH. The temperature of the solution is 25°C and the density is 1 g/mL. The enthalpy of neutralization for HCl and NaOH is -57.3 kJ/mol. Determine the heat of mixing for the solution.

asked Jan 22 in ThermoChemistry by IrwinDeBoos5 (610 points)

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1 answer 51 views

A sample of 55.0 g of ethanol at 25°C is vaporized at its normal boiling point. The enthalpy of vaporization for ethanol is 38.56 kJ/mol. Calculate the amount of heat energy required for this process.

asked Jan 22 in ThermoChemistry by DwainArreola (250 points)

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1 answer 6 views

A researcher is working on the desorption of a specific gas from a metal surface. The enthalpy of desorption for this process is -23.4 kJ/mol. If the researcher desorbs 0.75 moles of the gas, how much heat is released (or absorbed)?

asked Jan 22 in ThermoChemistry by AdolfoCarpen (270 points)

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1 answer 47 views

A piece of metal with a mass of 15 grams initially at 25°C is placed in 50 mL of water at 80°C. After the metal has reached thermal equilibrium with the water, its temperature is 30°C. Calculate the specific heat capacity of the metal.

asked Jan 22 in ThermoChemistry by Kimberly61S1 (630 points)

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1 answer 77 views

A chemistry student wants to prepare a solution that contains 25% ethanol (by volume) and the rest is water. The enthalpy of mixing for ethanol and water is -21.2 kJ/mol. How much heat is evolved when the student makes 500 mL of the solution?

asked Jan 22 in ThermoChemistry by MaddisonFarw (510 points)

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1 answer 57 views

A chemistry student wants to mix 50 mL of water at 25°C with 50 mL of ethanol at 25°C to make a solution. The heat of mixing for water and ethanol is -21.2 kJ/mol. Calculate the heat (in kJ) absorbed or released when the two liquids are mixed. (Assume the densities of water and ethanol are approximately 1 g/mL and 0.8 g/mL, respectively.)

asked Jan 22 in ThermoChemistry by Jannette93D8 (510 points)

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1 answer 78 views

A chemistry student wants to know the specific heat capacity of aluminum. The student has an aluminum block weighing 100 grams at a temperature of 20°C. The student heats the block until its temperature reaches 90°C by adding 500 Joules of heat. What is the specific heat capacity of aluminum?

asked Jan 22 in ThermoChemistry by Breanna4436 (550 points)

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1 answer 53 views

A chemistry student wants to determine the specific heat capacity of an unknown metal. The student performs a calorimetry experiment and records the following data: - 50 mL of water at 25°C was added to a calorimeter. - The initial temperature of the metal was 100°C. - The final temperature of the metal and water mixture was 30°C. - The mass of the metal was 100 grams.What is the specific heat capacity of the metal?

asked Jan 22 in ThermoChemistry by EsperanzaAch (570 points)

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1 answer 31 views

A chemistry student wants to determine the specific heat capacity of a metal sample. The student adds 50 g of the metal sample to 200 g of water at 25°C in a calorimeter. The temperature of the water rises from 25°C to 38°C. Assume the specific heat capacity of water is 4.184 J/g°C. What is the specific heat capacity of the metal sample?

asked Jan 22 in ThermoChemistry by ByronHedges2 (290 points)

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1 answer 70 views

A chemistry student wants to calculate the enthalpy of adsorption for the adsorption of nitrogen gas on a solid adsorbent. The student knows that the initial and final pressures of the nitrogen gas are 1 bar and 0.5 bar, respectively, and the surface area of the adsorbent is 2m^2/g. The student also has data on the temperature and the amount of nitrogen gas adsorbed on the adsorbent. Can you help the student calculate the enthalpy of adsorption?

asked Jan 22 in ThermoChemistry by YolandaBeard (430 points)

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1 answer 60 views

A chemistry student wants to calculate the enthalpy change (∆H) upon hydrolysis of magnesium chloride (MgCl2). The student knows that the enthalpy of formation (∆Hf) of MgCl2 is -641 kJ/mol and the enthalpy of formation of water (∆Hf) is -286 kJ/mol. The balanced chemical equation for the hydrolysis of magnesium chloride is MgCl2 + 2H2O → Mg(OH)2 + 2HCl. Calculate the enthalpy change (∆H) of this reaction.

asked Jan 22 in ThermoChemistry by TiffanySeeka (530 points)

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1 answer 42 views

A chemistry student wants to calculate the amount of heat required to melt 15 grams of ice at 0°C. Given that the enthalpy of fusion of ice is 6.01 kJ/mol, what is the total amount of heat required to completely melt the ice?

asked Jan 22 in ThermoChemistry by MagdaLanglai (610 points)

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1 answer 35 views

A chemistry student needs to determine the standard enthalpy change for the formation of NH3(g) from its constituent elements, using Hess's Law calculations. The student is given the following information:ΔHf°(NH3) = -46 kJ/molΔHf°(N2) = 0 kJ/molΔHf°(H2) = 0 kJ/molΔH298°(N2H4) = 95 kJ/molΔHf°(N2H4) = 50 kJ/mol2NH3(g) + N2H4(l) → 3N2(g) + 4H2(g)What is the value of ΔHf° for NH3, based on the above data?

asked Jan 22 in ThermoChemistry by PreciousS02 (710 points)

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1 answer 6 views

A chemistry student needs to determine the specific heat capacity of a metal block. The student has the following information: the mass of the block is 75 g and its initial temperature is 25°C. The student heats the block to 100°C, and calculates that it absorbed 1500 J of heat during this process. What is the specific heat capacity of the metal block?

asked Jan 22 in ThermoChemistry by ElliotTurnbu (450 points)

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1 answer 68 views

A chemistry student needs to determine the enthalpy of oxidation of magnesium. For this, they need to conduct an experiment in which they react 1 gram of magnesium metal with excess hydrochloric acid of 2 moles concentration. They need to measure the temperature change that occurs during the reaction, which they will use to calculate the enthalpy of oxidation of magnesium. What is the enthalpy of oxidation of magnesium according to the student's experiment?

asked Jan 22 in ThermoChemistry by Francis08376 (410 points)

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1 answer 67 views

A chemistry student needs to determine the enthalpy of desorption for a specific substance. The substance was adsorbed onto activated carbon in a packed bed reactor at 25°C and under a pressure of 4 bar. The adsorption process was carried out until saturation was reached. The packed bed reactor was then heated to 100°C until complete desorption. The pressure was maintained at 4 bar during the entire process. Given the initial mass of the adsorbate and the final mass of the activated carbon, calculate the enthalpy of desorption for the substance.

asked Jan 22 in ThermoChemistry by LilyBentley (330 points)

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