The addition of  1.250 g of zinc metal (65.38 g/mol) to 0.100 L of  0.1912  M HCl in a coffee-cup calorimeter causes the temperature to increase from 15.00°C to  21.95°C. What is the value of ΔHrxn for the following reaction? (Hint: Look at the reaction stoichiometry and decide which reactant is the limiting reactant.) Zn(s)+2HCl(aq)-->ZnCl2​(aq)+H2​(g) Assume the density and specific heat of the solution are 1.00 g/mL and 4.18 J/g·°C, respectively._____ kJ/mol reaction

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5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the temperature of the solution increases by 1.60oC. Calculate  ΔH for the reaction in kJ/mol of KOH .The specific heat capacity of the solution is 4.18 J/goC   ( Hint: the mass of the solution is 105g)      (Hint #2: is this + or -?) Your answer should be in kJ/mol and have 3 sig figs

Calculate ΔHrxn for the reaction: 7 C (s) + 8 H2 (g) → C7H16 (g) The following reactions and associated ΔHrxn values are may likely be helpful to you: Reaction A: C7H16(g) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (g) ΔHrxn = -4817 kJ Reaction B: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ Reaction C: 2 H2 (g) + O2 (g) → 2 H2O (g) ΔHrxn = -483.6 kJ

When 29.5 mL of 0.500 M H2SO4 is added to 29.5 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g · ° C.)

Given the information below, what is ΔGrxn for the reaction CO(g) → C(s) + ½ O2(g)?C(s) + O2(g) → CO2(g)     ΔGrxn = –394.4 kJCO(g) + ½ O2(g) → CO2(g)     ΔGrxn = –257.2 kJ

If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal).  In this reaction, we combine 5.85 g of 63.7 ºC water with 6.63 g of 18.9 ºC water in a calorimeter.  Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 28.8ºC.  Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water.  Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC.  The first law of thermodynamics tells us that all of these changes sum up to zero so   Enter your answer to one decimal place (tenths)

In a constant‑pressure calorimeter, 60.0 mL of 0.340 M Ba(OH)2 was added to 60.0 mL of 0.680 M HCl. The reaction caused the temperature of the solution to rise from 23.38 ∘C to 28.01 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g⋅°C,) respectively), what is Δ?ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. Δ?=         kJ/mol H2O

A sample of NaOH (MM = 40.00 g/mol) with a mass of 1.811 g was added to a solution of HNO3 in a coffee cup calorimeter for a final volume of 100.0 mL. If both solutions were initially at 24.5 °C and the temperature of the resulting solution was recorded as 27.0 °C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH. Assume that the density and the heat capacity of the resulting solution are the same as water, 1.00 g/mL and 4.184 J/(g x °C) respectively. Your Answer: Answer units