# Week 9 Tues quiz

## Quiz by Kari Stone

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8 questions
• Q1

Give the direction of the reaction, if K >> 1.

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300s
• Q2

Express the equilibrium constant for the following reaction.

N2(g) + 3 H2(g) ⇔  2 NH3(g)

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300s
• Q3

The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

H2(g) + Br2(g)  ⇌  2 HBr(g)  Kc = 3.8 × 104

2 HBr(g)  ⇌  H2(g) + Br2(g)  Kc =   ?

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300s
• Q4

The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant.

N2O4(g)  ⇌  2 NO2(g)           Kc = 1.46

3 N2O4(g)  ⇌  6 NO2(g)        Kc = ?

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300s
• Q5

What is Δn for the following equation in relating Kc to Kp?

N2(g) + 3 H2(g)  ⇌  2 NH3(g)

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300s
• Q6

The reaction below has a Kc value of 61.  What is the value of Kp for this reaction at 500 K?

N2(g) + 3 H2(g)  ⇌  2 NH3(g)

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300s
• Q7

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.

2 N2(g) + O2(g) ⇌ 2 N2O(g)

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300s
• Q8

Calculate the value of [N2]eq (in M) if [H2]eq = 2.0 M, [NH3]eq = 0.5 M, and Kc = 2.

N2(g) + 3 H2(g) ⇌ 2 NH3(g)

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