find the dH when 56g of AgNO3 (M = 169.9 g/mol) reacts. If the heat involved (derived from answer a) is transferred without loss to 100.0g of water at 25ºC. what is the final temperature of the water (CH2O = 4.18J/gºC)?

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A: Choose the equation that shows the correct relationship between their enthalpy changes--

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A:

Q: Calculate the enthalpy for this reaction: 2C(s) + H2(g) ---> C2H2(g)AH° = ??? kJ Given the following…

A:

Q: 1) Calculate the enthapy for the folowing reaction: Na(g) + 20(g) -> 2NO:(g) AH ??? kJ Using the…

A:

Q: Calculate the enthalpy change (in kJ) when 27.6 g of water vapor at 126.7 °C is converted to water…

A: Enthalpy change is calculated using formula: ∆H = - q  Where , q = heat    When water at 126.7 °C is…

Q: When 0.746 g of benzoic acid, C7H6O2 (122.12 g/mol) is burned in a bomb calorimeter, the temperature…

A: Given: massC7​H6​O2​=0.746g;MC7​H6​O2​​=122.12g/mol;Ti​=21.04°C;Tf​=23.90°CΔE=−3226kJ/molStep 1:…

Q: When 0.746 g of benzoic acid, C2H6O2 (122.12 g/mol) is burned in a bomb calorimeter, the temperature…

A: The number of moles of a substance can be calculated using the formula:n = m/Mwhere n is the number…

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A:

Q: Methane combusts via the following balanced reaction: CH4(g) + 2O2(g) --> CO2(g) + 2 H2O(g)…

A: Given that the gas is in 50.0 L container at 298 K and 1 atm. At STP 1 mole of gas occupies 22.4 L…

Q: The value of AH° for the reaction below is 128.1 kJ CH ,OH U - Co, 2(8) + 2H. 2(8) How may kJ of…

A: Given chemical equation is  CH3OH(l) -----> CO2(g) + 2H2(g) Enthalpy change, ∆H° = 128.1 kJ  We…

Q: Next, 4.490 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an…

A:

Q: Write the thermochemical equation for the following reactions that occur at constant pressure:  a)…

A: A thermochemical equation is a chemical equation which represents the enthalpy change of the…

Q: Enter your answer in the provided box. Consider the reaction H2g) + Ch@) → 2HCI(2) AH =-184.6 kJ/…

A:

Q: Consider the hypothetical case of removing the magnesium sulfate from solution and reforming the…

A: The heat energy released when new bonds are made between the ions/molecules and water molecules is…

Q: dont provide handwriting solution ....

A: Approach to solving the question:The standard enthalpies of formation are given:{eq}\Delta…

Q: 2. When 2.00 g of hydrazine (H,N2) decompose into 1.33 equivalents of NH3(8) and 1 equivalent of…

A: When 2.00 g of hydrazine N2H4 decompose into 1.33 equivalents of NH3(g) and 1 equivalent of N2(g) at…

Q: Assume that 100.0 mL of 0.200 M NaOH and 50.0 mL of 0.400 M HCl are mixed in a calorimeter. The…

A:

Q: 166. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a coffee cup…

A: The molar mass of water is 18.015 g/mol. The number of moles of water in the 40.0 g sample is…

Q: The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate…

A: Here we are required to find the Enthalpy change for the reaction.

Q: Consider the combustion of liquid CsHs in oxygen gas to produce carbon dioxide gas and water vapor.…

A: Balanced chemical equation :C5H8l + 7O2g →            5CO2g + 4H2Og∆H = -3068 kJmolCompound   ∆H°f…

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A: Given chemical equations:

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A:

Q: How much energy in kJ is released in burning 2.41 mL of gasoline (assuming that all of it is octane…

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Q: None

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A:

Q: THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the…

A: Enthalpy of reaction can be find by subtracting  sum of enthalpy of product from sum of enthalpy of…

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A:

Q: The combustion of 11.25 g of oxalic acid, C,H2O4 (s) in a bomb calorimeter whose heat capacity is…

A: given data is weight of oxalic acid is 11.25g heat capacity is 4.60KJ/0C temperature changes from…

Q: THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the…

A: The enthalpy can be calculated as:-

Q: For the reaction Na2CO3 (s) + 2HCI@) NaCle) + CO2 (9) + H2O) AH is -144.1 kJ. What is AU. O -141.62…

A:

Q: Given the heat of formation of the following compounds from their elemer AH°F = -393.5 kJ/mol CO:(g)…

A: The question is based on concept of chemical thermodynamics. We have to calculate enthalpy change…

Q: The overall reaction in a commercial heat pack can be represented as 4 Fe(s) +302 (9)→ 2 Fe,O,(s) AH…

A: Heat capacity of a substance or system indicates the amount of heat required to raise the…

Q: When 1.8 g of an unknown salt, A2B3 is added to a calorimeter containing 82 ml of water at 26.8 °C…

A: Given: volume of water = 82 mL. Mass of salt = 1.8 g. Change in temperature = -0.51 oC And the molar…

Q: 2) Why is AH used? Consider the following reaction taking place at constant temperature 298 K Na (s)…

A: The objective of the question is to determine  and and then find the percent difference from the…

Q: A process of synthesizing NH3 through the reaction: 3H¸ (g) + N (g) 2 2NH 2NH_(8) AGº(NH) 16500/…

A: The catalyst currently used in the Haber process:  Finely divided iron along with potassium…

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Q: The standard enthalpies of formation, at 25.00\deg C, of methane (CH4(g)), water (H2O(!), and carbon…

A:

Q: In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of 0.680 M HCI.…

A: no of mmoles of water produced is 34 mmoles. The total amount of heat produced is 1.937kJ so the…

Q: [References) The reusable booster rockets of the space shuttle use a mixture of aluminum and…

A: The balanced reaction taking place is given as, => 3 Al (s) + 3 NH4ClO4 (s) ---> Al2O3 (s) +…

Q: Determine ΔH in kJ/mol for the following reaction: 2NO(g) + O2(g) --> 2NO2(g) The standard…

A: Given that:  2NO(g) + O2(g) <......> 2NO2(g)  dH°NO = 90.4 KJ/mol  dH°NO2 = 33.9 KJ/mol

Q: Using the reaction enthalpy data shown, determine the amount of heat released in each situation: 2…

A: Stoichiometry, in balanced chemical reaction is defined by the ratio at which reactants are reacting…

Q: Consider the following thermochemical equations (Note: HA is a weak acid) H+(aq) + OH-(aq) → H2O(l)…

A: This question can be solved using Hess's law of constant heat summation.