5. A 1.058-g sample of benzoic acid (HC;H;O2) is completely combusted in a "bomb" calorimeter, and the temperature of the calorimeter increases from 21.50°C to 28.45°C. The calorimeter contains 750.0 g of water (specific heat = 4.184 J/g.°C) and the "bomb“ has heat capacity of 890. J°C. Calculate: (a) the amount of heat (in kJ) absorbed by water; (b) the amount of heat (in kJ) absorbed by the "bomb"; (c) the total amount of heat (in kJ) produced by the combustion of benzoic acid sample, and (d) the molar enthalpy of combustion (AHcomb; in kJ/mol) of benzoic acid. (Answer: (a) 21.8 kJ; (b) 6.19 kJ; (c) -28.0 kJ; (d) AH.comb = -3.23 x 10° kJ/mol)

Please help me with the attached question.

12. Consider the following process. AH = -802 kJ + 202 (2) 2 CO2 (g) + 2H,O(3) CHAIB) + 2H,O(g) A) Is the reaction exothermic or endothermic? B) What is the enthalpy change for the following reaction? + H2O(e) 1/2CH4 () + O2 () O 1/2 CO2 (8) + H,0R)

Given the following equation and the molar enthalpy of combustion of methane gas:                  CH4((g)  +  2O2(g)  -->  CO2(g)  +  2H2O(g);    DHocomb = -802.5 kJ    How many grams of water can be heated from 20.0oC to 100.0oC using the heat produced by the complete combustion of 5.00 g of methane gas (CH4; molar mass = 16.04 g/mol)? The specific heat of water is 4.184 J/g.K          (A) 747 g          (B) 598 g          (C) 201 g          (D) 0.747 g

O 437.0 kJ O 256.0 kJ 103.6 kJ O-103.6 kJ

Tetrachloromethane, CCl4, is formed from methane and chlorine in the following reaction: CH4 (g) + 4 Cl₂ (g) → 4 HCl(g) + CCl4 (g) = Calculate A₁H, the enthalpy change for this reaction, using the enthalpies of formation of CO₂ (g), H₂O(l), and CCl4 (g), (▲ƒ H° = enthalpy changes for the following reactions: CH4 (g) + 2 O2(g) → 2 H₂O(l) + CO₂(g) ΔΗ° :-890.4 kJ/mol-rxn 2 HCl(g) → H₂(g) + Cl₂ (g) ΔΗ° +184.6 kJ/mol-rxn = ΔΗ° = Compound AfH (kJ/mol) H₂O(g) CO₂(g) -285.8 -393.5 kJ/mol-rxn - 95.98 kJ/mol), and the

1. Calculate the enthalpy of reaction for the combustion of methane gas, CH4, to form CO,(g) + H,O(1).

In this problem you are going to determine the molarity of a strong acid solution by measuring the enthalpy change of the acid’s reaction with a base, which causes the temperature of the reaction mixture to go from 22.3 °C to 34.8 °C. You will have to look up values from your OpenStax text. A)  What is the underlying reaction of every acid-base neutralization reaction? What is the enthalpy change of this reaction per mole of acid? B) You performed this acid-base neutralization reaction with 100.0 mL of 2.00 M sodium hydroxide (base) and 60.0 mL of your unknown strong acid. What is the total volume of your reaction mixture after you mix the two solutions together? (The base is in excess.)

when octane (C8H18) is burned under standard conditions, the enthalpy of combustion is -5698.34KJ / mol. Using the information provided. what is the heat of formation of octane?

There are all one question. Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) 2Hg(l) + O2(g)2HgO(s)......ΔH° = -181.6 kJwhat is the standard enthalpy change for the reaction:(3) PbO(s) + Hg(l)Pb(s) + HgO(s)......ΔH° = ? _______kJ   Given the standard enthalpy changes for the following two reactions:(1) 4C(s) + 5H2(g)C4H10(g)...... ΔH° = -125.6 kJ(2) C2H4(g)2C(s) + 2H2(g)......ΔH° = -52.3 kJwhat is the standard enthalpy change for the reaction:(3) 2C2H4(g) + H2(g)C4H10(g)......ΔH° = ? ______kJ   Given the standard enthalpy changes for the following two reactions:(1) N2(g) + O2(g)2NO(g)...... ΔH° = 181.8 kJ(2) N2(g) + 2O2(g)N2O4(g)......ΔH° = 9.2 kJwhat is the standard enthalpy change for the reaction:(3) 2NO(g) + O2(g)N2O4(g)......ΔH° = ? ______kJ