Equations Flashcards

1
Q

State the equation for moles in solution.

A

m = c * v

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2
Q

State the equation for moles from mass.

A

moles = mass / mr

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3
Q

state the ideal gas eqation with units.

A

P(pa)V(m3) = nRT(k)

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4
Q

State the equation for percent atom economy.

A

%AE = 100*(sum of products mr / sum of reactant mr)

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5
Q

State the equation for q

A

q = mc*ΔT

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6
Q

State the equation for enthalpy change from with q

A

ΔH = -q / moles

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7
Q

State the rate equation

A

Rate = k[A]^m [B]^n

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8
Q

State the arrhenius equation

A

k = Ae^ (-Ea/RT)

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9
Q

State the equation for lnk as y=mx+c

A

lnk = -Ea/R * 1/T + lnA

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10
Q

State the equation for activation energy.

A

Ea = RT * (lnA-lnK)

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11
Q

State the half equations within a rechargeble cell.

A

Positive electrode: Li+ + CoO2 + e- -> Li+[CoO2]-
Negative electrode: Li -> Li+ + e-

Li + + CoO2 -> Li+[CoO2]-

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12
Q

State the definition of pH

A

pH = -log10[H+]

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13
Q

State the ionic product of water and its value at 27oc 1

A

Kw = [H+][OH-]

10^-14

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14
Q

State the equation for Ka and pKA

A
Ka = ([H+][A-])/[HA]
ka = 10^-pKa
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15
Q

State the equation for the reaction between sulfric acid and sodium chloride

A

NaCl(s) + H2SO4(l) -> NaHSO4(s) + HCl(g)

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16
Q

State the equation for the reaction between bromide and sulfric acid

A

2H+ + 2Br- + H2SO4(l) -> SO2(g) + 2H2O(l) + Br2(g)

17
Q

State the equation for the reaction between iodide ions and sulfric acid.

A

8H+ + 8I- + H2SO4(l) -> H2S(g) + 4H2O + I2

18
Q

State the equation for silver ions and chloride.

A

Cl-(aq) + Ag+(aq) -> AgCl(s)

19
Q

State the equation for silver ions and bromide.

A

Br-(aq) + Ag+(aq) -> AgBr(s)

20
Q

State the equation for silver ions and iodidie.

A

I-(aq) + Ag+(aq) -> AgI(s)

21
Q

State the equation for silver ions and carbonate ions

A

2Ag+(aq) + CO3 2-(aq) -> Ag2CO3(s)

22
Q

State the equation for silver ions and hydroxide ions.

A

Ag+(aq) + OH-(aq) -> AgOH(s)

23
Q

State the equation for % error

A

% error = (uncertainty(max error) / measured) * 100

24
Q

State the equation for the thermal demomposition fo NaHCO3

A

2 NaHCO3 → Na2CO3 + H2O + CO

25
Q

State the equation for enthalpy change.

A

ΔH = sum of H products - sum of H reactants

26
Q

State the equation for entropy change

A

ΔS = sum of S products - sum of S reactants.

27
Q

State the equation for gibbs free energy

A

ΔG = ΔH - TΔS

28
Q

State the equation for chlorine reacting with water

A

Cl2(aq) + H2O(l) HClO(aq) + HCl(aq)
this is driven to completion
Cl2(aq) + 2H2O(l) -> 4HCl(aq) + O2(g)

29
Q

State the equation for sodium hypochlorite and water.

A

NaClO(s) + H2O(l) Na+(aq) + OH-(aq) + HClO(aq)

30
Q

state the eqation for the reation between chlorine and sodium hydroxide.

A

Cl2(g) + 2NaOH(aq) -> NaClO(aq) + NaCl(aq) + H2O(l)

31
Q

State the equation for the thermal decomposition of calcium carbonate.

A

CaCO3(s) -> CaO(s) + CO2(g)

32
Q

State the eqaution for the reaction between CaO and HCl

A

CaO(s) + 2HCl(aq) ->CaCl2(aq) + H2O(l)

33
Q

State the eqaution for the reaction between Ca(OH)2 and HCl

A

Ca(OH)2(s) + 2HCl(aq) -> CaCl2(aq) + 2H2O