First Law Fundamentals

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Fundamental energy conservation

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Saipreeti Gouripeddi

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First Law Fundamentals


First Law FundamentalsVersión en línea Fundamental energy conservation por Saipreeti Gouripeddi 1 If an isolated system undergoes a process, what is ΔU (change in internal energy)? a Undefined b Negative c Positive d Zero 2 Zeroth law implies what about thermal equilibrium and temperature? a Temperature has no relation to equilibrium b Only solids reach equilibrium c Equilibrium is not transitive d If A is in equilibrium with B and B with C, then A is in equilibrium with C 3 Which quantity is a state function: internal energy, heat, or work? a Heat b Internal energy c Work d Temperature 4 Numerical: A system receives q = 500 J and does w = -200 J of work on the surroundings. Find ΔU. a +300 J b -300 J c 0 J d +200 J 5 Which best describes a system versus its surroundings? a System is the entire universe b Both terms mean the same thing c System is the part of the universe under study; surroundings are everything else d Surroundings are the system’s boundary 6 In the first law, which convention is commonly used: q in = heat added to system; w by system = work done by system? a Yes; q is heat added to system and w is work done by system b No; q is heat released and w is work done on the system c Only enthalpy is used in the first law d Both q and w are always zero 7 Which statement best defines equilibrium in thermodynamics? a A process currently occurring at maximum rate b A state where macroscopic properties are unchanging with time absent external forces c A state of zero energy d A state of maximum temperature 8 For an ideal gas in an isothermal process, what is ΔU? a Zero b Negative c Positive d It depends on volume change 9 Which is a true statement about state functions? a They are always equal to heat exchanged b They depend only on the current state, not on path taken c They depend on the process path d They are always equal to zero Feedback 1 In an isolated system, q=0 and w=0, so ΔU = q + w = 0. 2 Thermal equilibrium is transitive; equal temperatures imply mutual equilibrium. 3 State functions depend only on the state, not on the path; internal energy is a state function. 4 ΔU = q + w; 500 + (-200) = 300 J. 5 The system is what you analyze; surroundings are everything else beyond its boundary. 6 Common convention: q in (positive for heat added), w by system (positive for work done by system). 7 Equilibrium means no net macroscopic change without external influence. 8 For an ideal gas, internal energy depends only on temperature; isothermal means T constant, so ΔU = 0. 9 State functions like U, H, S depend only on state, not the path.

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First Law Fundamentals

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First Law FundamentalsVersión en línea

por Saipreeti Gouripeddi

If an isolated system undergoes a process, what is ΔU (change in internal energy)?

Zeroth law implies what about thermal equilibrium and temperature?

Which quantity is a state function: internal energy, heat, or work?

Numerical: A system receives q = 500 J and does w = -200 J of work on the surroundings. Find ΔU.

Which best describes a system versus its surroundings?

In the first law, which convention is commonly used: q in = heat added to system; w by system = work done by system?

Which statement best defines equilibrium in thermodynamics?

For an ideal gas in an isothermal process, what is ΔU?

Which is a true statement about state functions?

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