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What is a equation that is the inverse of the exponential equation?
Logarithmic equation
What is the equation of this question?
The equation is "What = ?"
What is x in this equation?
what is the equation
How do you put equation in a sentence?
"Figure out this mathematical equation" "This is how to figure out an equation" "An equation is something widely used in mathematics."
What is the term used for a quantity which when substituted for the unknown quantity in an equation satisfies the equation?
It is the solution to the equation or a root of the equation.
What is a chemical reaction at equilibrium?
deltaG = deltaH -TdeltaS. deltaG = 0 at equilibrium. Therefore deltaH = TdeltaS
What is the balanced chemical equation Nabh4 plus h20 yield NaBo plus h2?
NaBH4 + 2H2O -> NaBO2 + 4H2 [1] DeltaG(298K)= -299 kJ/mol BH4 DeltaH(298K)= -231 kJ/mol BH4 (10.8 mass% H) NaBH4 + 4H2O -> NaB(OH)4 + 4H2 [2] DeltaG (298K)= -315 kJ/mol BH4 DeltaH = -247 kJ/mol BH4 (7.28 mass% H) NaBH4 + 6H2O -> NaB(OH)4.2H2O [3] DeltaG = -319kJ/mol BH4 DeltaH = -213 kJ/mol BH4 (5.48 mass% H) *Hydrolysis in Eq.[1] is not the most favorable reaction!
If a reaction has an enthalpy of -54.32 kJ/mol and an entropy of -354.2 J/(K*mol), what is the Gibbs free Energy at 54.3(degrees c)?
DeltaG = DeltaH - TDeltaS dG = -54.32 kJ/mol - (54'32+273)K(-354.2J/molK) NB Thevtemperature is quoted in Kelvin(K) and the Entropy must be converted to kJ by dividing by '1000'/ Hence dG = - 54.32kJ/mol - (327.32K)(-0.3542 kJ/molK) NB The 'K' cancels out. Then maker the multiplication dG = -54/32 kJ/mol - - 115.94 kJ/mol Note the double minus; it becomes plus(+). Hence dG = -54.32kj/mol + 115.94 kJ/mol dG = (+)61.61 kJ/mol Since dG is positive, the reaction is NOT thermodynamically feasible.
What does a negative deltaH tell about a reaction?
the reaction is exothermic
What important information does a thermochemical equation have that a regular balanced equation does not?
A thermochemical equation shows the amount of heat given out or taken in when the reaction occurs. CH4 + 2O2 = CO2 +2H2O, deltaH = -890 kJ/mol Note delta H is negative when heat is given out, exothermic and +ve when endothermic. Sorry can't do delta symbol - its a triangle!
Which of the following is endothermic a dry ice evaporating b a sparkler burning c the reaction that occurs in a chemical cold pack often used to ice athletic injuries?
Dry ice evaporating is endothermic-->+DeltaH A sparkler burning is exothermic--->-DeltaH The reaction that occurs in a chemical cold pack often used to ice athletic injuries is endothermic--->+DeltaH
The reaction between strontium metal and chlorine gas is described by the following thermochemical equation Sr s Cl2 g plus SrCl2 s deltaH -829 kJ mol-1 What will be the enthalpy change to 2 sig figs?
-830
What is thermo and half cells?
•deltaG = nFE • •Pt + In3+ > In + Pt2+ •Pt > Pt2+ + 2e- •In3+ +3e- > In
What important information does thermochemical equation have that a regular balanced equations does not?
A thermochemical equation shows the amount of heat given out or taken in when the reaction occurs. CH4 + 2O2 = CO2 +2H2O, deltaH = -890 kJ/mol Note delta H is negative when heat is given out, exothermic and +ve when endothermic. Sorry can't do delta symbol - its a triangle!
What is S in the equation delta G equals delta H minus TdeltaS?
The change in enthalpy between products and reactants in a reaction
How can an unknown deltaH reaction be determined using Hess's law?
Enthalpies from reaction steps are added to determine an unknownHreaction.
How do you calculate voltage using Nernst equation?
The Nernst equation is E = ((-2.3RT)/zF)*(log10 [Ci/Co])E = equilibrium potential (mV)z = charge on the ion(2.3RT)/F = constant (60mV at 37C)Ci = intracellular concentrationCo = extracellular concentrationThe Nernst equation is important because it shows what the equilibrium potential would be for one ion.E.g. The resting membrane potential is normally ~70mV. So during an action potential Na channels open their gates briefly and Na rush inside the cell. Na is ionized and carries a positive charge. So when Na rushes into the cell it makes the inside of the cell more positive. If you were to break off the gate and allow Na to move freely back and forth, the Nernst equation shows us that the equilibrium point for Na is ~+65mV.•deltaG - DG0 = R T ln Q• deltaG = nFE••••E = E0+ (RT / nF) ln Q
