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MrRa [10]
3 years ago
7

What is the final temperature of the solution formed when 1.52 g of NaOH is added to 35.5 g of water at 20.1 °C in a calorimeter

? NaOH (s) → Na+ (aq) + OH– (aq) ∆H = -44.5 kJ/mol
Chemistry
1 answer:
Inessa [10]3 years ago
4 0

Answer : The final temperature of the solution in the calorimeter is, 31.0^oC

Explanation :

First we have to calculate the heat produced.

\Delta H=\frac{q}{n}

where,

\Delta H = enthalpy change = -44.5 kJ/mol

q = heat released = ?

m = mass of NaOH = 1.52 g

Molar mass of NaOH = 40 g/mol

\text{Moles of }NaOH=\frac{\text{Mass of }NaOH}{\text{Molar mass of }NaOH}=\frac{1.52g}{40g/mole}=0.038mole

Now put all the given values in the above formula, we get:

44.5kJ/mol=\frac{q}{0.038mol}

q=1.691kJ

Now we have to calculate the final temperature of solution in the calorimeter.

q=m\times c\times (T_2-T_1)

where,

q = heat produced = 1.691 kJ = 1691 J

m = mass of solution = 1.52 + 35.5 = 37.02 g

c = specific heat capacity of water = 4.18J/g^oC

T_1 = initial temperature = 20.1^oC

T_2 = final temperature = ?

Now put all the given values in the above formula, we get:

1691J=37.02g\times 4.18J/g^oC\times (T_2-20.1)

T_2=31.0^oC

Thus, the final temperature of the solution in the calorimeter is, 31.0^oC

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What type of chemical reactions are molecules joined together to form more complex molecules?
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Anabolic reaction are specific type of reaction in which molecules joined together to form more complex molecules.

Explanation:

Metabolic reactions are catagorized into 2 types

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3 0
3 years ago
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3 0
2 years ago
How many moles of sodium will react with water to produce 2.0 mol of hydrogen in the following reaction?
ser-zykov [4K]

Answer: 4.0 moles of sodium will react with water to produce 2.0 mol of hydrogen

Explanation:

The balanced chemical equation is:

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According to stoichiometry :

1 mole of H_2 is produced by = 2 moles of Na

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4 0
2 years ago
How many moles are in 8.5 x 1023 molecules of co?
natulia [17]
<h3>Answer:</h3>

1.4 mol CO

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

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

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

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

8.5 × 10²³ molecules CO

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

Avogadro's Number

<u>Step 3: Convert</u>

  1. Set up:                    \displaystyle 8.5 \cdot 10^{23} \ molecules \ CO(\frac{1 \ mol \ CO}{6.022 \cdot 10^{23} \ molecules \ CO})
  2. Divide:                    \displaystyle 1.41149 \ mol \ CO

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

1.41149 mol CO ≈ 1.4 mol CO

7 0
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