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igomit [66]
3 years ago
7

How much heat is gained when a 50.32g piece of aluminum is heated from 9.0°c to 16°c

Chemistry
2 answers:
Rashid [163]3 years ago
5 0

Answer: 317 joules

Explanation:

The quantity of heat energy (Q) gained by aluminium depends on its Mass (M), specific heat capacity (C) and change in temperature (Φ)

Thus, Q = MCΦ

In this case,

Q = ?

Mass of aluminium = 50.32g

C = 0.90J/g°C

Φ = (Final temperature - Initial temperature)

= 16°C - 9°C = 7°C

Then, Q = MCΦ

Q = 50.32g x 0.90J/g°C x 7°C

Q = 317 joules

Thus, 317 joules of heat is gained.

morpeh [17]3 years ago
4 0

Answer: 317 joules

Explanation:

The quantity of heat energy (Q) gained by aluminium depends on its Mass (M), specific heat capacity (C) and change in temperature (Φ)

Thus, Q = MCΦ

In this case,

Q = ?

Mass of aluminium = 50.32g

C = 0.90J/g°C

Φ = (Final temperature - Initial temperature)

= 16°C - 9°C = 7°C

Then, Q = MCΦ

Q = 50.32g x 0.90J/g°C x 7°C

Q = 317 joules

Thus, 317 joules of heat is gained.

PLEASE MARK AS THE BRAINIEST ANSWERED AS I HAVE JUST ANSWERED THIS FOR YOU

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2Mg + O2 → 2MgO<br><br> If you are burning 5.8332 g of Mg, how many grams of MgO will this make?
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<h3>Answer:</h3>

9.6724 g MgO

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

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<u>Step 1: Define</u>

[RxN - Balanced] 2Mg + O₂ → 2MgO

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

[RxN] 2 mol Mg = 2 mol MgO

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Molar Mass of O - 16.00 g/mol

Molar Mass of MgO - 24.31 + 16.00 = 40.31 g/mol

<u>Step 3: Stoichiometry</u>

  1. Set up:                              \displaystyle 5.8332 \ g \ Mg(\frac{1 \ mol \ Mg}{24.31 \ g \ Mg})(\frac{2 \ mol \ MgO}{2 \ mol \ Mg})(\frac{40.31 \ g \ MgO}{1 \ mol \ MgO})
  2. Multiply/Divide:                                                                                               \displaystyle 9.67241 \ g \ MgO

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 5 sig figs.</em>

9.67241 g MgO ≈ 9.6724 g MgO

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