Do Now - AP - Calculate Constants/Concentration/Partial Pressure

When the following reaction reached equilibrium,

SO_{2 (g)} + NO_{2 (g)} <=> SO_{3 (g)} + NO (g)

there was 0.40 M SO₃, 0.30 M NO, 0.15 M NO₂, and 0.20 M SO₂.

Calculate the equilibrium constant for this reaction.

• 4.0

• 0.42

• 0.25

• 1.0

Tags

NGSS.HS-PS1-6

If a K value is greater than 1,

• more products are present at equilibrium

• more reactants are present at equilibrium

When performing equilibrium calculations, what would you use to solve for x?

• a cubic equation

• desmos graphing calculator

• a quadratic equation

• an exponential equation

The E line on a ICE table is simply just ___

• the amount of unknown

• the sum of the initial line and the change line

• the equivalent parts per million

• the energy change

Tags

NGSS.HS-PS1-4

What is written on the C line of a ICE table?

• how much of each substance will change during the reaction

• the concentrations of each substance

• ideal gas constants

• the chemical formulas for each reactant and product

What is written on the I line of a ICE table?

• independent variables

• the initial concentrations of each substance

• ideal gas constants

• the balanced chemical equation of reaction

Find the K_c for
2NOBr_(g) + Cl_2(g) ↔ 2NO_(g) + 2BrCl_(g)
 if 

2NOBr_(g) ↔ 2NO_(g) + Br_2(g) has a K_c = 0.014
Br_2(g) + Cl_2(g) ↔ 2BrCl_(g) has a K_c = 7.2

• 0.1008

• 7.214

• 514

• 0.00194

• 1 x 10^-20

• 1 x 10^-10

• 1 x 10¹⁰

• 1 x 10²⁰

2 SO_2(g) + O_2(g) ↔ 2 SO_3(g)

When 0.40 M SO₂ and 0.60 M O₂ are placed in a flask, the reaction represented above occurs. After the reaction reaches equilibrium, the flask is found to contain 0.30 mole of SO₃.

(Use an ICE chart to help you determine the values to plug into the K_c expression)

• 
• 
• 
• 

Answer explanation

2 SO_2(g) + O_2(g) ↔ 2 SO_3(g)

_{I 0.40M 0.60M 0M}

_{C -2x -x +2x}

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E 0.30

solve for x and then determine SO₂ and O₂

go back and plug into the K_c equation

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-5

NGSS.HS-PS1-7

CH₄(g) + CO₂(g) ↔ 2 CO(g) + 2 H₂(g)

A 1.00-L flask is filled with 0.30 mol of CH₄ and 0.40 mol of CO₂, and allowed to come to equilibrium. At equilibrium, there are 0.20 mol of CO in the flask. What is the value of K_c, the equilibrium constant, for the reaction?

(Use and ICE table to help you determine the values at equilibrium to plug into the K equation)

• 1.2

• 0.027

• 0.30

• 0.060

• 3.0