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CHEM 1001 Study Guide - Midterm Guide: Ideal Gas Law, Bond Energy, Photon

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1 Oct 2018

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CHEM 1001 Full Course Notes

CHEM 1001 Full Course Notes

Document Summary

Answer each of the six questions with a few sentences or equations where necessary. (5 marks each) Unless we have a perfect insulator between the experiment and the surroundings, heat will flow from the laboratory into the experiment, raising the temperature of the experiment. Beginning with nis(s), show the three reactions leading to acid rain. Nis(s) + 3/2 o2(g) nio + so2(g) A measurement at constant pressure yields the enthalpy change of the system. This is different from the internal energy change of the system by an amount p v. This reaction has only two moles of substance of the left and 12 on the right. This equation connects the two ideas of the nature of light, i. e. that it has wavelike properties such as frequency ( ) as well as particle like properties such as energy per photon (e). Which of the following five sets of quantum numbers are allowed and which are not? n.

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Related Questions

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.