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2 years ago

How much heat is required to convert 29g of ice at -4.0c to water vapor at 105

Chemistry

1 answer:

kumpel [21]2 years ago

7 0

Answer:

45 degrees at 29 so 105 is lower than 45 and 105 wants to be 32 so 45 can be higher. so then the water vapor will be 35 because 105 is too much of water gallon

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What is the difference between qualitative data and quantitative data?

astraxan [27]

Quantitative data can be counted, measured, and expressed using numbers. Qualitative data is descriptive and conceptual.

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2 years ago

What sequence should be followed when conducting a laboratory investigation? Make observations, gather experimental data, form a

AURORKA [14]

Answer:

Define a problem, form a hypothesis, gather experimental data, form a conclusion

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3 years ago

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Tamoxifen is a drug used to prevent recurrence of certain types of breast cancers that require estrogen to grow. Tamoxifen binds

fredd [130]

Answer:

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Explanation:

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2 years ago

The lock-and-key mechanism refers to

miskamm [114]

Answer:

A). The complementary shapes of an enzyme and a substrate.

Explanation:

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3 years ago

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Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfe

Vesna [10]

Answer:

In the given chemical reaction:

Species Oxidized: I⁻

Species Reduced: Fe³⁺

Oxidizing agent: Fe³⁺

Reducing agent: I⁻

As the reaction proceeds, electrons are transferred from I⁻ to Fe³⁺

Explanation:

Redox reaction is a chemical reaction involving the simultaneous movement of electrons thereby causing oxidation of one species and reduction of the other species.

The chemical species that gets reduced by gaining electrons is called an oxidizing agent. Whereas, the chemical species that gets oxidized by losing electrons is called a reducing agent.

Given redox reaction: 2Fe³⁺ + 2I⁻ → 2Fe²⁺ + I₂

Oxidation half-reaction: 2 I⁻ + → I₂ + 2 e⁻ ....(1)

Reduction half-reaction: [ Fe³⁺ + 1 e⁻ → Fe²⁺ ] × 2

⇒ 2 Fe³⁺ + 2 e⁻ → 2 Fe²⁺ ....(2)

In the given redox reaction, Fe³⁺ (oxidation state +3) accepts electrons and gets reduced to Fe²⁺ (oxidation state +2) and I⁻ (oxidation state -1) loses electrons and gets oxidized to I₂ (oxidation state 0).

Therefore, Fe³⁺ is the oxidizing agent and I⁻ is the reducing agent and the electrons are transferred from I⁻ to Fe³⁺.

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