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andreev551 [17]
3 years ago
10

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3 At this temp, 0.3000 mol of H2 and 0.300 mol o

f I2 were placed in a 1L container to react. What concentration of HI is present at equilibrium? H2+I2<-> 2HI
Chemistry
1 answer:
Vlada [557]3 years ago
4 0
Your answer is: Kc = [HI]² / {[H2] [I2]} 
<span>53.3 = (2x)² / {(0.400M - x)(0.400M - x)} </span>
<span>sqrt(53.3) = 2x / (0.400M - x) </span>
<span>2.92 - 7.30x = 2x </span>
<span>x = 0.314M </span>

<span>[HI] = 2x = 0.628M

:) hopefully this helped. (:</span>
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gulaghasi [49]
<h3>Answer:</h3>

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<h3>General Formulas and Concepts:</h3>

<u>Math</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

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<u>Stoichiometry</u>

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<h3>Explanation:</h3>

<u>Step 1: Define</u>

[Given] 5.61 moles CO₂

[Solve] molecules CO₂

<u>Step 2: Identify Conversions</u>

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<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                      \displaystyle 5.61 \ mooles \ CO_2(\frac{6.022 \cdot 10^{23} \ molecules \ CO_2}{1 \ mol \ CO_2})
  2. [DA] Multiply/Divide [Cancel out units]:                                                          \displaystyle 3.37834 \cdot 10^{24} \ molecules \ CO_2

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

3.37834 × 10²⁴ molecules CO₂ ≈ 3.38 × 10²⁴ molecules CO₂

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