Below is the reaction for the evaporation of water: H20 (1) → H20 (g) AH°f H2O (1)= -285.8 kJ/mole; H20 (g) = -241.8 kJ/mole %3D Calculate AH°rxn for this process. This is the reaction that happens when your sweat evaporates. Why is this a cooling mechanism for your body? How much sweat would have to evaporate from a persons skin to cool the body by 0.5°C? Assume this person has a body mass of 150 Ibs and the specific heat capacity of the body is 4.0 J/g °C. 1 lb. = 0.454 kg

Consider the following reaction at 25 °C: 3 Ni(s) + N₂(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH3(g) If AG° = 18.1 kJ/mol, determine the value of AG assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N₂ and 10.07 atm of H₂O.

Consider four 100.0-g samples of water, each in a separate beaker at 25.0 °C. Into eachbeaker you drop 10.0 g of a different metal that has been healed to 95.0 °C. Assumingno heat loss to the surroundings, which water sample will have the highest finaltemperature? Explain your answer.l type='a'>The water to which you have added aluminum °C).i>The water to which you have added iron °C)i>The water to which you have added copper °C).i>The water to which you have added lead °C).i>Because the masses of the metals are the same, the final temperatures would be thesame.

The overall reaction in a commercial heat pack can be represented as 4 Fe(s) + 30₂(g) → 2 Fe₂O₂ (s) AH = -1652 kJ a. How much heat is released when 4.80 moles of iron are reacted with excess O₂? Heat = kJ b. How much heat is released when 1.00 mole of Fe2O3 is produced? Heat = kJ c. How much heat is released when 1.40 g iron is reacted with excess O₂? Heat = kJ d. How much heat is released when 11.4 g Fe and 1.90 g O₂ are reacted? Heat = kJ Submit Answer Retry Entire Group 9 more group attempts remaining

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18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation:  O2 = 0.00  kJ / mole,  H2O (g) = -245 kJ / mole,   CO2 = -318 kJ/mole  and  C3H8  = -438 kJ / mole C3H8 = 44.09 g/mole  Temperature is 33 oC a. -789 kJ b. -212 kJ c. 412 kJ d. -169 kJ

A 104.4mL sample of 1.8M HNO3 is mixed with a 800mL sample of 0.5M KOH in a Styrofoam cup. If both solutions were initially at 25.2\deg C, and the enthalpy of the neutralization reaction is -57 kJ/mole of H2O formed, what is the final temperature of the mixture? The volume of the formed H2O can be ignored. Assume that the solution has a density of 1.00 g/mL and a specific heat of 4.184 J/g\deg C, and that the Styrofoam cup has an insignificant heat capacity. (enter one decimal place)

The value of AH° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed. 26. CH4 (g) + 3Cl, (g) → CHC1; (1) + 3HC1 (g) A) B) C) 211 177 70.7 D) -336