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3 years ago

10. Write the formula for the compounds: copper (1) chloride and copper (II) chloride

Chemistry

1 answer:

Natali [406]3 years ago

3 0

Answer:

Copper(II) chloride (CuCl2) reacts with several metals to produce copper metal or copper(I) chloride (CuCl) with oxidation of the other metal.

Explanation:

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Anna35 [415]

Answer:

The respiratory system is the network of organs and tissues that help you breathe. basically your airways, lungs, and blood vessels so you quite literally need these to survive I mean your muscles need oxygen to function and your brain needs oxygen to function so without your respiratory system you wouldn't be able to move much and you would quickly pass out and die from the lack of oxygen to your brain there are other body processes that need oxygen as well but these are just two examples.

Explanation:

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3 years ago

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You are given a sample of limestone, which is mostly CaCO3, to determine the mass percentage of Ca in the rock. You dissolve the

irakobra [83]

Answer:

34.15% is the mass percentage of calcium in the limestone.

Explanation:

Mass of precipitate that is calcium oxalate = 140.2 mg = 0.1402 g

1 mg = 0.001 g

Moles of calcium oxalate = $\frac{0.1402 g}{128 g/mol}=0.001095 mol$

1 mole of calcium oxalate have 1 mole of calcium atom.

Then 0.001095 moles of calcium oxalate will have 0.001095 moles of calcium atom.

Mass of 0.001095 moles of calcium :

0.001095 mol × 40 g/mol = 0.04381 g

Mass of sample of limestone = 128.3 mg = 0.1283 g

Percentage of calcium in limestone:

$\frac{0.04381 g}{0.1283 g}\times 100=34.15\%$

34.15% is the mass percentage of calcium in the limestone.

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3 years ago

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Lab: Limiting Reactant and Percent Yield

creativ13 [48]

Answer : If a substance is the limiting reactant, then it limits the formation of products because in the reaction it is present in limited amount.

Explanation :

While observing a chemical reaction, we can tell about whether a reactant is limiting or excess.

Step 1 : first write the chemical reaction and then balanced the chemical equation.

$C_2H_4+H_2\rightarrow C_2H_6$

Step 2 : convert the given masses into the moles if mass of $C_2H_4$ is 10.5 g and molar mass of $C_2H_4$ is 28 g/mole and the mass of hydrogen is 0.40 g and molar mass of hydrogen is 2 g/mole.

$\text{moles of }C_{2}H_{4}=\frac{10.5g}{28g/mole}=0.375moles$

$\text{moles of }H_{2}=\frac{0.40g}{2g/mole}=0.20moles$

Step 3 : Now we have to determine the limiting reagent and excess reagent.

$\text{ moles of }C_{2}H_{4}\text{ in excess}=0.375-0.20=0.175\text{moles}$

Now we conclude that $C_{2}H_{4}$ is the limiting reagent and hydrogen is an excess reagent.

Hypothesis :

Limiting reagent : It is the reagent in the chemical reaction that is totally consumed when the chemical reaction is complete. Limiting reagent limits the formation of products.

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2 years ago

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Why is thre no gas bubble whene there is citric acid?answer all the questions in detail.

kaheart [24]

Answer:

This is because the carbon dioxide gas that dissolved in the water is not very soluble. ... After the citric acid solution and baking soda react, carbon dioxide gas is formed, along with other products.

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2 years ago

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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3 years ago