A balloon filled with 39.1 mol of helium has a volume of 876 L at 0.0 ℃ and 1.00 atm pressure. At constant pressure, the temperature of the balloon is increased to 38.0 ℃ causing the balloon to expand to a volume of 998 L. calculate q, w, and ∆? for the helium in the balloon. (The molar heat capacity for helium gas is 20.8 J ℃-1 mol -1)

ir A sample of glass, which has a specific heat capacity of 0.670 J.g .°C *, is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The glass sample starts off at 92.3 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 25.0 °C. The pressure remains constant at 1 atm. sa Calculate the mass of the glass sample. Be sure your answer is rounded to 2 significant digits. Explanation Check Terms of Use 02021 McGraw Hill LLC. All Rights Reserved Address

Calculate ∆E for each of the following.a. q = −47 kJ, w = + 88 kJb. q = +82 kJ, w = −47 kJc. q = + 47 kJ, w = 0d. In which of these cases do the surroundings do work on the system

Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat.C(s) + O2(g) ------->CO2(g) ∆H° rxn = -393.5 k

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 6.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 44.66 °C over a time of 14.6 minutes. Next, 4.910 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 40.44 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of…

Consider a balloon filled with 2115 L of helium at 1.00 atm pressure and 45.5°C. The temperature of the balloon is decreased to 26.3°C with the pressure remaining at 1.00 atm. What is ∆E (in kJ) for this change? (Assume ideal conditions. The molar heat capacity for He at constant pressure, Cp, is 20.8 J/°C･mol.)

2 NO(g) + O2(g) ––––> 2 NO2(g); ∆H° = –114.4 kJ Given the thermochemical equation above, how much heat is given off by the system when 951.1 g of NO2 is produced? (the molar mass of NO2 is 46.00 g/mol) A) 114.4 kJ B) 1.183 x 103 kJ C) 2.365 x 103 kJ D) 5.534 kJ E) 1.088 x 105 kJ

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 51.74 °C over a time of 14.9 minutes. Next, 4.510 g of ethane (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 53.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ per mole of C₂H6.…

Hw.77.

Energy in the amount of 5.0 J is added to 0.50 g pieces of aluminum, copper, and magnesium that are initially kept at 22 °C. The molar heat capacities of these metals are 24.3 J/(mol·°C), 24.5 J/(mol·°C), and 24.9 J/(mol·°C), respectively. Which piece of metal will have the highest temperature and what is that temperature?