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This Concept Map, created with IHMC CmapTools, has information related to: ncope, ΔU The change in the internal energy of the gas. ΔU=(3/2)nRΔT, First Conservation of Energy for Thermodynamic Processes ΔU=Q+W, PV=nRT Gay-Lussac's, ΔU=Q+W Q, PV=nRT Combined, PV=nRT Charles', Boyle's Contant Temperature <math xmlns="http://www.w3.org/1998/Math/MathML"> <mrow> <mmultiscripts> <mtext> P </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mrow> <mmultiscripts> <mtext> V </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> = </mtext> <mrow> <mmultiscripts> <mtext> P </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mrow> <mmultiscripts> <mtext> V </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> </mrow> </mrow> </mrow> </mrow> </math>, Charles' Contant Pressure <math xmlns="http://www.w3.org/1998/Math/MathML"> <mrow> <mtext> ( </mtext> <mmultiscripts> <mtext> V </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> )=( </mtext> <mrow> <mmultiscripts> <mtext> V </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ) </mtext> </mrow> </mrow> </mrow> </mrow> </math>, Q Heat flowing into the system Q=n(Constant variable)ΔT, ΔU=Q+W W, Second It is impossible for any process to have as its sole result the transfer of heat from a cooler to a hotter body., Laws Zeroth, Gay-Lussac's Constant Volume <math xmlns="http://www.w3.org/1998/Math/MathML"> <mrow> <mtext> ( </mtext> <mmultiscripts> <mtext> P </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> )=( </mtext> <mrow> <mmultiscripts> <mtext> P </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ) </mtext> </mrow> </mrow> </mrow> </mrow> </math>, PV=nRT Boyle's, Laws First, ΔU=Q+W ΔU, Combined Same substance under diff. conditions <math xmlns="http://www.w3.org/1998/Math/MathML"> <mrow> <mtext> ( </mtext> <mmultiscripts> <mrow> <mmultiscripts> <mtext> P </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> V </mtext> </mrow> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 1 </mtext> <none/> </mmultiscripts> <mtext> )=( </mtext> <mrow> <mmultiscripts> <mrow> <mmultiscripts> <mtext> P </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> V </mtext> </mrow> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ÷ </mtext> <mrow> <mmultiscripts> <mtext> T </mtext> <mtext> 2 </mtext> <none/> </mmultiscripts> <mtext> ) </mtext> </mrow> </mrow> </mrow> </mrow> </math>, Laws Ideal Gas, W Work done on the system by the envoronment W=-PΔV, Laws Second