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3 years ago

If there are 4 grams of product produced by the chemical reaction, how many grams of reactant were consumed?

Chemistry

2 answers:

Colt1911 [192]3 years ago

8 0

D 4 grams
i need to write a couple more character for explanation so there

sasho [114]3 years ago

8 0

Hey there!

 If there are 4 grams of product produced by the chemical reaction, how many grams of reactant were consumed?

Answer: 
) 4 grams

Hope this helps
Have a great day (:

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2 years ago

How many km are in 5.6mm? 5.6x103 5.6x10-6 5.6x10-3 5.6x106

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Hey there :)

Question: How many km are in 5.6mm?

=>5.6x10^3

=>5.6x10^-6

=>5.6x10^-3

=> 5.6x10^6

Answer:-

$5.6 \times 10^{ - 6}$

Explanation:-

By using the formula-

$1millimeter = \frac{1}{1000000}$

As 1 with 6 zeros, we convert it into exponential form.

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Now combine with given question.

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2 years ago

How would Bohr model show the protons in a carbon atom

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Answer:

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According to Bohr's model of the atoms, the Rutherford model is basically correct. This implies that Bohr model accepts the idea of a nucleus containing nucleons(protons and neutrons).

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A graphic description of this is shown in the image attached to this answer.

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2 years ago

An analytical chemist weighs out 0.093g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with

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Answer:

The molar mass of the unknown acid is 89 g/mol

Explanation:

Step 1: The balanced equation

HA(aq) + NaOH(aq) → NaA(aq) + H2O(l)

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

Step 2: Data given

Mass of the acid = 0.093 grams

volume = 250 mL

titrates with 0.16 M NaOH

adds 6.5 mL NaOH

Step 3: Calculate moles of NaOH

We know the concentration and volume of NaOH needed to neutralize the acid.

By determining the moles of NaOH in that volume in liters (95.9mL=0.0959L), the moles of acid in the original sample can be determined from the reaction stoichiometry.

Moles = Molarity * Volume

Moles = 0.16 M * 0.0065 L

Moles = 0.00104 moles NaOH

Step 4: Calculate moles of the unknown acid:

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

For 0.00104 moles NaOH we have 0.00104 moles of HA

Step 5: Calculate the molar mass of the acid

Molar mass Ha = Mass Ha / moles Ha

Molar mass Ha = 0.093 grams / 0.00104 moles

Molar mass Ha = 89.42 g/mol ≈89 g/mol

The molar mass of the unknown acid is 89 g/mol

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3 years ago