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3 years ago

Which two energy sources were used the most in

Chemistry

1 answer:

Naily [24]3 years ago

4 0

Answer:

The 1st and 2nd ones on the top

Explanation:

Hope this helps:)

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2ch4(g) c2h2(g) 3h2(g) describe what is happening within the system when it is at equilibrium in terms of concentrations, reacti

SashulF [63]

Balanced chemical reaction: 2CH₄(g) ⇄ C₂H₂(g) + 3H₂(g).

1) In a chemical reaction, chemical equilibrium is the state in which both reactants (methane CH₄) and products (ethyne C₂H₂ and hydrogen H₂) are present in concentrations which have no further tendency to change with time.

2) At equilibrium, both the forward and reverse reactions are still occurring.

3) Reaction rates of the forward and backward reactions are equal and there are no changes in the concentrations of the reactants and products.

4 0

3 years ago

Read 2 more answers

What is definition "scientific question"?

Lemur [1.5K]

Answer:

A scientific question is basically a question that can lead to a hypothesis to help us figure out the observation in science. I hope this helps you

4 0

2 years ago

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When 11.12 g of neon is combined in a 100 L container at 80oC with 9.59 g of argon, what is the mole fraction of argon?

PolarNik [594]

The correct answer for the question that is being presented above is this one: "0.3."

Here it is how to solve.
Molecular mass of Ar = 40
Molecular mass of Ne = 20
Number of moles of Ar = 9.59/40 = 0.239
Number of moles of Ne = 11.12/20= 0.556
Mole fraction of argon = 0.239/ ( 0.239 + 0.556) = 0.3

3 0

3 years ago

How many liters are present in 10 grams of H2O ?

Luba_88 [7]

Answer:

About 0.01

Explanation:

1 grams of H2O = 0.0010

0.0010 x 10 = 0.01

8 0

3 years ago

CH4 + O2 → CO2 + H2O

Scilla [17]

Answer:

9.8 × 10²⁴ molecules H₂O

General Formulas and Concepts:

Atomic Structure

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

Organic

Naming carbons

Stoichiometry

Analyzing reaction rxn
Using Dimensional Analysis

Explanation:

Step 1: Define

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

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

[Given] 130 g CH₄

Step 2: Identify Conversions

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

Step 3: Stoichiometry

[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]: $\displaystyle 9.75526 \cdot 10^{24} \ molecules \ H_2O$

Step 4: Check

Follow sig fig rules and round. We are given 2 sig figs.

9.75526 × 10²⁴ molecules H₂O ≈ 9.8 × 10²⁴ molecules H₂O

8 0

2 years ago