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andre [41]
3 years ago
5

Will the energy released in the synthesis of water equal the energy absorbed in the decomposition of water?

Chemistry
1 answer:
mariarad [96]3 years ago
6 0

Answer:

yes

Explanation:

the energy released in the synthesis of water is equal to the energy absorbed in the decomposition of water. This outcome happens because the difference in energy between the reactants and the products in both cases is equal. . It follows the law of conservation of energy.

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How many moles of solute are contained in a 250 ml solution that has a concentration of.85 m?
oksano4ka [1.4K]
Volume = 250 mL in liters : 250 / 1000 => 0.25 L

Molarity = 0.85 M

Number of moles:

n = M x V

n = 0.85 x 0.25

n = 0.21 moles

Choice B
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3 years ago
What bonds break? select that apply
igor_vitrenko [27]
Hydrogen-Hydrogen
Oxygen=Oxygen
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Consider that the room is a closed system. Ryan uses the chemical energy in his muscles to create the energy of motion. He uses
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D.

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A 24.00 mL sample of a solution of Pb(ClO3)2 was diluted with water to 52.00 mL. A 17.00 mL sample of the dilute solution was fo
klio [65]

Answer:

0.238 M

Explanation:

A 17.00 mL sample of the dilute solution was found to contain 0.220 M ClO₃⁻(aq). The concentration is an intensive property, so the concentration in the 52.00 mL is also 0.220 M ClO₃⁻(aq). We can find the initial concentration of ClO₃⁻ using the dilution rule.

C₁.V₁ = C₂.V₂

C₁ × 24.00 mL = 0.220 M × 52.00 mL

C₁ = 0.477 M

The concentration of Pb(ClO₃)₂ is:

\frac{0.477molClO_{3}^{-} }{L} \times \frac{1molPb(ClO_{3})_{2}}{2molClO_{3}^{-}} =0.238M

4 0
3 years ago
How much energy is lost to condense 300. grams of steam at 100.C?
True [87]

Energy lost to condense = 803.4 kJ

<h3>Further explanation</h3>

Condensation of steam through 2 stages:

1. phase change(steam to water)

2. cool down(100 to 0 C)

1. phase change(condensation)

Lv==latent heat of vaporization for water=2260 J/g

\tt Q=300\times 2260=678000~J

2. cool down

c=specific heat for water=4.18 J/g C

\tt Q=300\times 4.18\times (100-0)=125400

Total heat =

\tt 678000+125400=803400~J

3 0
2 years ago
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