Zumdahl Chemistry Chapter 4, 5, 6, 10, 18 All Needed Equations

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45 Terms

1
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Molarity Equation

M=mol/L

2
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1 atm

101,325 Pa

101.325 kPa

760 mmHg

760 torr

14.7 psi

1.01 bar

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Van Der Waals Equation

[Pobs + a(n/V)^2](V - nb) = nRT

4
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Ideal Combined Gas Law

(P1V1/n2T2) = (P2V2/n2T2)

5
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Boyle’s Gas Law

P1V1 = P2V2

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Charle’s Gas Law

(V1/T1) = (V2/T2)

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Avogadro’s Gas Law

(V1/n1) = (V2/n2)

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Real Gas Law

Pobs + a(n/V)2(V-nb) = nRT

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Ideal Gas Law

PV = nRT

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Density Ideal Gas Law

d = (PM/RT)

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Molar Mass of A Gas Equation

M = (dRT/P)

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Mole Fraction

X1 = (n1/nTotal) = (n1/n1 + n2 + n3 + n…)

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Dalton Law of Partial Pressures

PTotal = P1 + P2 + P3 + …

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Pressure and Volume (Boyle’s Law)

P = (nRT)(1/V)

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Pressure and Temperature (Ideal Gas Law)

P = (nR/V)T

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Volume and Temperature (Charles’s Law)

V = (nR/P)T

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Volume and Number of Moles (Avogadro's Law)

V = (RT/P)n

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STP gasses

22.4 L/mol

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Non-STP gasses

PV = nRT

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Density of Water

1.00 g/mL or 1000 g/L

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Constant Pressure Calorimetry

qsoln = msoln cs,soln ΔT

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Energy of Reaction Using Calorimetry

qrxn = -qsoln

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Calorimetry With Multiple Substances

qsoln + qsoln =-q3

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Isochoric (Constant Volume)

  1. ΔU = ±Q

  2. ΔV = 0

  3. W = 0

  4. Q = nCvΔT

P1/T1 = P2/T2

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Isobaric (Constant Pressure)

  1. ΔU = ±q ±w

  2. ΔP = 0

  3. W = PΔV

    • W = nRΔT

  4. Q = nCpΔT

  5. ΔV = nCvΔT

    • V1/T1 = V2/T2

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Isothermal (Constant Temperature)

  1. W = ±Q

    • W = nRT * ln(Vf/Vi)

  2. ΔT = 0

  3. Q = W

    • Q = nRT * ln(Pi/Pf)

  4. ΔV = 0

    • P1/V1 = P2/V2

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Adiabatic (No Heat Flow)

  1. CV = 3/2 R

  2. W = -nCVΔT

  3. Q = 0

  4. ΔU = ±W

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Internal Energy of System

U = ±Q ∓W

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Cautious-Clapeyron Equation at 1 Temperature

Loge(P) = -Delta H/RT

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Cautious-Clapeyron Equation at 1 Temperature Enthalpy Derivative

Delta H = -Lne(P)[(RT)]

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Cautious-Clapeyron Equation at 2 Temperature

Loge(P T1/P T2) = Delta H/R (1/T2 - 1/T1)

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Cautious-Clapeyron Equation at 1 Temperature Temperature Derivative

T = -{[Lne(P)](R)}/Delta H

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Cautious-Clapeyron Equation at 2 Temperature 2nd Pressure Derivative

P2={e^[(Delta Hvap/R)(1/T2 - 1/T1)]}/P1

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Cautious-Clapeyron Equation at 2 Temperature Enthalpy Derivative

P2={e^[(Delta Hvap/R)(1/T2 - 1/T1)]}/P1

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Root Mean Squared Velocity Equation

Sqrt{[(8.314J*mol^-1*K-1)(Temperature)]/(M in kg/mol)}

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Diffusion Equation

R1/R2 = sqrt(M2/M1)

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Effusion Equation

R = sqrt(1/M)

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pH Equation

pH = -log[H+]

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pOH Equation

pOH = -log[OH-]

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pOH Equation

pH = -log[H+]

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pH to molar concentration

10^-pH

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pOH to molar concentration

10^-pOH

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Sum of pH and pOH

pH + pOH = 14

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Cautious-Clapeyron Equation at 2 Temperature 2nd Temperature Derivative

T2 = [(1/T1) - RLoge(P T1/P T2)/Delta Hvap]^-1

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Gas Constant (R)

8.314 J*mol^-1*K^-1

0.08206 L*atm*mol^-1*K^-1