Does the temperature outside affect how fast molecules move inside objects? Charles Law helps us understand how molecules move in different temperatures. It states that increasing the temperature of a constant pressure volume of gas causes individual gas molecules to move faster (Andrew Staroscik Staroscik 9/19/16)‚ and the volume is proportional to the absolute temperature of a gas at (Todd Helmenstine 10/16/16). Therefore‚ as the temperature increases‚ so does the speed of the molecules‚ and when
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dynamic method to measure the ratio of the specific heat capacities of air and‚ in the second‚ you will investigate the behaviour of gas undergoing an expansion that is approximately adiabatic and ‘partially reversible’ – somewhere between the two limits of a completely irreversible (free) and perfectly reversible expansion. The air can be considered an ideal gas. DESCRIPTION AND EXPERIMENTAL PROCEDURE PART I: Determination of γ for Air Motion of Steel ball steel ball R Tap ubber mat The
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theory to explain the following: i)Matter can exist in three states ii)The pressure exerted by a confined gas decreases as its temperature is lowered iii)A gas of low molecular mass will diffuse through air faster than a gas of high molecular masseven though both are at same temperature. The Kinetic Theory can be used to describe the three physical states of matter namely‚ solid‚ liquid and gas. In this theory‚ some basic assumptions has to be made: a) all matter is made up of extremely small particles
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Theory: An ideal gas obeys the equation of state that the pressure‚ specific volume or density‚ and absolute temperature with mass of molecule and the gas constant‚ R. PV = mRTM Where‚ P = Absolute pressure V = Volume n = Amount of substance (moles) R = Ideal gas constant T = Absolute temperature (K) However‚ real gas does not absolutely obey the equation of state. A few changes on the ideal gas equation of state allow its application in the properties of real gas. When energy
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I O N B Answer at least TWO (2) Questions from this Section 4. (a) (i) What is an ideal gas? (2 marks) (ii) Write the ideal gas equation and give the units used for each term in the equation when R = 0.0821L-atm/mol-K. (3 marks) (b) Why was this equation modified and what is the modified form of the equation? (5 marks) (c) Calculate‚ using the modified equation‚ the pressure at which one mole of chlorine gas will occupy 22400 cm3 at 0oC. (For chlorine‚ a = 6.49 L2-atm/mol and b = 0.0562L/mol
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Topic 1.2 AMOUNT OF SUBSTANCE The mole Reacting masses and atom economy Solutions and titrations The ideal gas equation Empirical and molecular formulae Ionic equations Mill Hill County High School THE MOLE Since atoms are so small‚ any sensible laboratory quantity of substance must contain a huge number of atoms: 1 litre of water contains 3.3 x 1025 molecules. 1 gram of magnesium contains 2.5 x 1022 atoms. 100 cm3 of oxygen contains 2.5 x
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pieces of ham and 20 pieces of bread? 20B x 1S = 10S 21H x 1S=7S 2B 3H The smaller of answer from the 2 givens is the answer. The reactant that produced the smaller amount is called the limiting reactant. (in this case‚ ham) Part IV: Gas Laws
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projected problems and requests your assistance on the particular one described below. Decades from now‚ the present method of supplying energy to households (i.e.‚ with electricity‚ gas‚ or o11) may not be possible. Instead‚ housepersons will shop for their energy in supermarkets (Figure P4.5). Cyhnders of gas (let us ? +llh ’ I Figure P4.5 assume that the cylinders contain air) may be purchased and connected to any number of Carnot engines or other such efficient devices to be
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S53718/7 © UCLES 2004 [Turn over 2 Data speed of light in free space‚ permeability of free space‚ permittivity of free space‚ elementary charge‚ the Planck constant‚ unified atomic mass constant‚ rest mass of electron‚ rest mass of proton‚ molar gas constant‚ the Avogadro constant‚ the Boltzmann constant‚ gravitational constant‚ acceleration of free fall‚ c = 3.00 × 10 8 m s –1 0 0 =4 × 10 –7 H m–1 = 8.85 × 10 –12 F m–1 e = 1.60 × 10 –19 C h = 6.63 × 10 –34 J s u = 1.66 × 10 –27 kg
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thermal equilibrium with the surroundings‚ which are at 15oC. Determine the final pressure in the tank. (4 marks) Figure 1 5. Nitrogen at 150 K has a specific volume of 0.041884 m3/kg. Determine the pressure of the nitrogen‚ using (a) the ideal gas equation and (b) the Beattie-Bridgeman equation. Compare your results to the experimental value of 1000 kPa. (9 marks) Date of submission: 19th October 2011 (EH2211A)/20th October 2011
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