CHEM 203 Study Guide - Midterm Guide: Reagent, Kinematics, Bayerischer Rundfunk

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amaranthdonkey808

20 Apr 2019

School

University of Calgary

Department

Chemistry

Course

CHEM 203

Professor

Bronwen Wheatley

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Document Summary

Equilibrium: kp = kc ( rt ) " n. A n ( c t d ) ca t b ) If equilibrium goes the previous of from fwd. If an equation is multiplied by a raised number same to the s rev then just take the reciprocal coefficient then the kc needs to be. Kc: when adding equilibrium equations together , multiply the kc values ! : q: calculated in the same way k is calculated , but products and reactants are not at equilibrium c- tf. I rates ? e g s s l. How to: rates of measure rates reaction are always positive ! ( rates of appearance 1 disappearance can be. Instantaneous rate = slope of tangent line to that point (cid:8869) in time initial rate instantaneous rate @ e - Overall reaction order is the sum of all the exponents. Rate = kea ] m [ b) n.

Related Questions

The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation

Kp=Kc(RT)În

where R=0.08206 Lâ atm/(Kâ mol), T is the absolute temperature, and În is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction

N2(g)+3H2(g)â2NH3(g)

for which În=2â(1+3)=â2.

Part A

For the reaction

2A(g)+2B(g)âC(g)

Kc = 60.2 at a temperature of 59 âC .

Calculate the value of Kp.

Part B

For the reaction

X(g)+2Y(g)â2Z(g)

Kp = 2.17Ã10^â2 at a temperature of 39 âC .

Calculate the value of Kc.