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GREYUIT [131]
3 years ago
14

N writing a chemical equation that produces hydrogen gas, the correct representation of hydrogen gas is

Chemistry
1 answer:
andrezito [222]3 years ago
4 0
Need more information
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How many neutrons are in 7.00 g of 13c?
Minchanka [31]
You multiply the number of atoms by 12 to get how many electrons (since each atom has 12 electrons in it)
you multiply the number of atoms by 13 to get how many neutrons
(since each atom of this isotope has 13 neutrons in it)
5 0
3 years ago
Which of the following has the largest radius?<br><br><br> Answer:K
mixas84 [53]

Answer:

the answer is k? lol thanks

4 0
3 years ago
The reactants of two chemical equations are listed.
hjlf
The correct answer is b
8 0
3 years ago
Determine the volume of a 0.800 M K2Cr2O7 solution required to completely react with 4.24 g of Cu.
Pachacha [2.7K]

<u>Answer:</u> The volume of solution required is 0.0275 L.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of copper = 4.24 g

Molar mass of copper = 63.55 g/mol

Putting values in above equation, we get:

\text{Moles of copper}=\frac{4.24g}{63.55g/mol}=0.067mol

The chemical equation for the reaction of potassium dichromate and copper follows:

K_2Cr_2O_7+3Cu+7H_2SO_4\rightarrow 3CuSO_4+Cr_2(SO_4)_3+K_2SO_4+7H_2O

By Stoichiometry of the reaction:

3 moles of copper reacts with 1 mole of potassium dichromate.

So, 0.067 moles of copper will react with = \frac{1}{3}\times 0.067=0.022mol of potassium dichromate

To calculate the volume of potassium dichromate, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

We are given:

Moles of potassium dichromate = 0.022 mol

Molarity of solution = 0.800 M

Putting values in above equation, we get:

0.08mol/L=\frac{0.022mol}{\text{Volume of solution}}\\\\\text{Volume of solution}=0.0275L

Hence, the volume of solution required is 0.0275 L.

6 0
3 years ago
You are asked to prepare 500. mL 0.150 M acetate buffer at pH 5.10 using only pure acetic acid ( MW = 60.05 g/mol, p K a = 4.76
Amanda [17]

Answer:

4.504g of acetic acid

Explanation:

The acetic acid in reaction with NaOH produce acetate ion, thus:

CH₃COOH + NaOH → CH₃COO⁻ + H₂O + Na⁺

<em>That means the moles of acetate buffer comes, in the first, from the acetic acid</em>

As you need 500mL (0,500L) of a 0.150M acetate buffer, moles are:

0.500L × (0.150mol / 1L) = <em>0.075 moles of acetate</em>. That is:

0.075mol = [CH₃COO⁻] + [CH₃COOH]

Thus, grams of acetic acid you need to prepare the buffer are:

0.075 moles acetic acid × (60.05g / 1mol) = <em>4.504g of acetic acid</em>

6 0
3 years ago
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