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CHEM101 Lecture Notes - Lecture 16: Calorimeter, Ideal Gas, Calorimetry

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30 Oct 2018

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Glennys O'Brien

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At a constant pressure, measures the heat of reaction (in a insulated coffee cup ) At a constant volume, the (cid:3247)bomb calorimeter(cid:3248) measures the internal energy change u, Thermally insulating, usually for combustion reactions, and heat capacity of calorimeter must be known, . Open system exchange of both matter and energy with surroundings. Closed system fixed amount of matter but energy can be exchanged with the surroundings. Relationship between h (heat change) and u (energy change) Bomb calorimeter and coffee cup measure two slightly different things. For reactions where no gas is produced or consumed, little expansion work will be done, hence the difference between and h and u will be negligible so we can assume that they equal each other. But if a gas is formed, work is done, and then need to use the ideal gas equation to relate the.

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Related Questions

Calorimetry is a method used to measure changes inenthalpy, or heat, that occur during chemical processes. Two commoncalorimeters are constant-pressure calorimeters and constant-volume(or "bomb") calorimeters. Bomb calorimeters are used to measurecombustion and other gas-producing reactions, in which the reactionis observed in a strong, sealed vessel. A simple constant-pressurecalorimeter can be made from a foam coffee cup and a thermometer,in which energy changes in a reaction are observed via the changein temperature of the solution in the cup. The idea behindcalorimeters is that if they are sufficiently insulated from theoutside environment, any energy gained or lost in the chemicalreaction will be directly observable as a temperature and/orpressure change in the calorimeter.

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Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V Assuming constant pressure, rank these reactions from most energy released by the system to most energy absorbed by the system, based on the following descriptions: Surroundings get colder and the system decreases in volume. Surroundings get hotter and the system expands in volume. Surroundings get hotter and the system decreases in volume. Surroundings get hotter and the system does not change in volume. Also assume that the magnitude of the volume and temperature changes are similar among the reactions. Rank from most energy released to most energy absorbed. To rank items as equivalent, overlap them. Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g) + 4Y(g) - 2Z(g), Delta H degree = -75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L Calculate the value of the total energy change. AE, in kilojoules. Express your answer with the appropriate units.