How much energy (heat) is required to convert 33.5 g of H2O(l) at 8.7°C to H2O(g) at 129.3°C? specific heat of ice: 2.09 J/g·°C specific heat of water: 4.184 J/g·°C specific heat of steam: 1.84 J/g·°C ΔHfus = 6.02 kJ/mol ΔHvap = 40.7 kJ/mol Answer = ___________kJ

Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C6H6) from 0.00 °C to 99.3 °C molar mass: 78.11 g/mol cs,solid  = 1.51 J/g*°C cs,liquid  = 1.70 J/g*°C cs,gas  = 1.05 J/g*°C ΔHfus = 9.9 kJ/mol ΔHvap = 33.8 kJ/mol Tf = 5.6°C Tb = 80.08°C

Diethyl ether, used as a solvent for extraction of organic compounds from aqueous solutions, has a high vapor pressure which makes it a potential fire hazard in laboratories in which it is used. How much energy is released when 315.0 g is cooled from 153.0°C to 0.0°C? boiling point: 34.5°C Heat of vaporization: 351 J/g Specific heat capacity, (CH3)2O(l): 3.74 J/(g·K) Specific heat capacity, (CH3)2O(g): 2.35 J/(g·K) 145 kJ 158 kJ 116 kJ 63.1 kJ 21.1 kJ

The following is the balanced equation for the reaction of gaseous ammonia with oxygen gas.                       4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g)   Using the ΔHf° values shown below, calculate the ΔHrxn° for the overall reaction.        ΔHf°(NO (g)) = 91.3 kJ/mol      ΔHf°(NH3 (g)) = −45.9 kJ/mol      ΔHf°(H2O (l)) = −241.8 kJ/mol A) −294.8 kJ/mol B) −731.5 kJ/mol C) −902.0 kJ/mol D) −468.2 kJ/mol

Chloromethane, CH3 Cl, arises from microbial fermentation and is found throughout the environment. It is also produced industrially, is used in the manufacture of various chemicals, and has been used as a topical anesthetic. How much energy is required to convert 86.0 g of liquid to a vapor at its boiling point, -24.09 °C? (The heat of vaporization of CH3 Cl is 21.40 kJ/mol.) Energy required = kJ

6. Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C. What was the initial temperature change of the ice? The specific heat capacity of H20(s) = 2.1 J/(g.°C).

The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol

A (4.1700x10^1) g sample of water (C = 4.18 J / g ºC) initially is at (5.110x10^1)ºC. What is the final temperature of this water in ºC if it loses (3.39x10^3) J of heat?

A sample of steam with a mass of 0.529 g at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °c. (For water, AHvap = 40.7 kJ/mol and Cwater = 4.18 J/(g · °C).) - Part A Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using three significant figures.

You have 500 g of dry ice at a temperature of 50 K. How much energy would it take to produce carbon dioxide gas heated to a temperature of 400оC?   Specific heat of CO2(s) = 0.709 J/g K     Specific heat of H2O(s) = 2.040 J/g K Specific heat of CO2(g) = 0.850 J/g K                             Specific heat of H2O(l) = 4.184 J/g K Specific heat of H2O(g) = 2.010 J/g K Freezing point (CO2) = -78.5оC                                                          Freezing point (H2O) = 273.15 K Latent heat of sublimation (CO2) = 199 J/g Latent heat of fusion (H2O) = 334 J/g     Latent heat of vaporization (H2O) = 2260 J/g