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3 years ago

If the temperature of 1000 mL of gas is changed from -86oC to 101oC. What is the approximate final volume?

Chemistry

1 answer:

valentinak56 [21]3 years ago

5 0

Answer:

2000 mL

Explanation:

We have the following data:

Initial volume: V₁ = 1000 mL

Initial temperature: T₁ = -86°C + 273 = 187 K

Final temperature: T₂= 101°C + 273 = 374 K

According to Charles' law, as the temperature of a gas is increased at constant pressure, the volume is increased. That is expressed mathematically as:

V₁/T₁ = V₂/T₂

Thus, we calculate the final volume V₂ as follows:

V₂ = V₁/T₁ x T₂ = (1000 mL)/187 K x 374 K = 2000 mL

Therefore, the final volume is 2000 mL.

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<h3>What is meant by Perhydrol?</h3>

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<h3>What is Merck's Perhydrol?</h3>

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2 years ago

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Ahat [919]

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3 years ago

CH4 + O2 → CO2 + H2O

Scilla [17]

Answer:

9.8 × 10²⁴ molecules H₂O

General Formulas and Concepts:

<u>Atomic Structure</u>

Reading a Periodic Table
Moles
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Organic</u>

Naming carbons

<u>Stoichiometry</u>

Analyzing reaction rxn
Using Dimensional Analysis

Explanation:

<u>Step 1: Define</u>

[RxN - Unbalanced] CH₄ + O₂ → CO₂ + H₂O

[RxN - Balanced] CH₄ + 2O₂ → CO₂ + 2H₂O

[Given] 130 g CH₄

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

Avogadro's Number

[RxN] 1 mol CH₄ → 2 mol H₂O

[PT] Molar Mass of C: 12.01 g/mol

[PT] Molar Mass of H: 1.01 g/mol

Molar Mass of CH₄: 12.01 + 4(1.01) = 16.05 g/mol

<u>Step 3: Stoichiometry</u>

[DA] Set up conversion: $\displaystyle 130 \ g \ CH_4(\frac{1 \ mol \ CH_4}{16.05 \ g \ CH_4})(\frac{2 \ mol \ H_2O}{1 \ mol \ CH_4})(\frac{6.022 \cdot 10^{23} \ molecules \ H_2O}{1 \ mol \ H_2O})$
[DA] Divide/Multiply [Cancel out units]: $\displaystyle 9.75526 \cdot 10^{24} \ molecules \ H_2O$

<u>Step 4: Check</u>

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

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