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Archy [21]
3 years ago
6

What is the concentration of a solution formed by mixing 89.94 grams of cobalt (II)

Chemistry
2 answers:
gulaghasi [49]3 years ago
6 0

Answer:

M=0.467M

Explanation:

Hello,

In this case, cobalt (II) molar mass is 280.996 g/mol since it is about heptahydrate, so we compute the moles:

n=89.94g*\frac{1mol}{280.996g}= 0.32mol

Then, since we need the volume in litres only:

V=68.6cL*\frac{1L}{100cL} =0.686L

Finally, we compute the molarity:

M=\frac{0.32mol}{0.686L}\\ \\M=0.467M

So your answer should be refined.

Best regards.

bezimeni [28]3 years ago
3 0

Answer:

0.47 M

Explanation:

The concentration of the solution can be calculated using the following equation:

C = \frac{\eta}{V} = \frac{m}{M*V}

<u>Where:</u>

V: is the volume of the solution = 68.6x10⁻² L

η: is the moles of cobalt (II)  sulfate

m: is the mass of cobalt (II)  sulfate = 89.94 g

M: is the molar mass of cobalt (II)  sulfate = 281.103 g/mol

The concentration of cobalt (II)  sulfate is:

C = \frac{m}{M*V} = \frac{89.94 g}{281.103 g/mol*68.6 \cdot 10^{-2} L} = 0.47 mol/L

We used the molar mass of the cobalt (II)  sulfate heptahydrate (281.103 g/mol) since it is one of the most common salts of cobalt.

Therefore, the concentration of a solution of cobalt (II)  sulfate is 0.47 M (assuming that the cobalt (II)  sulfate is heptahydrate).

I hope it helps you!

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Answer:

sodium chloride

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2 years ago
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Excess magnesium reacts with 165.0 grams of hydrochloric acid in a single displacement reaction.
JulsSmile [24]

Answer:

The volume of hydrogen gas produced will be approximately 50.7 liters under STP.

Explanation:

Relative atomic mass data from a modern periodic table:

  • H: 1.008;
  • Cl: 35.45.

Magnesium is a reactive metal. It reacts with hydrochloric acid to produce

  • Hydrogen gas \rm H_2, and
  • Magnesium chloride, which is a salt.

The chemical equation will be something like

\rm ?\;Mg\;(s) + ?\;HCl \;(aq)\to ?\;H_2 \;(g)+ [\text{Formula of the Salt}],

where the coefficients and the formula of the salt are to be found.

To determine the number of moles of \rm H_2 that will be produced, first find the formula of the salt, magnesium chloride.

Magnesium is a group 2 metal. The oxidation state of magnesium in compounds tends to be +2.

On the other hand, the charge on each chloride ion is -1. Each magnesium ion needs to pair up with two chloride ions for the charge to balance in the salt, magnesium chloride. The formula for the salt will be \rm MgCl_2.

\rm ?\;Mg\;(s) + ?\;HCl\;(aq) \to ?\;H_2 \;(g)+ ?\;MgCl_2\;(aq).

Balance the equation. \rm MgCl_2 contains the largest number of atoms among all species in this reaction. Start by setting its coefficient to 1.

\rm ?\;Mg\;(s) + ?\;HCl\;(aq) \to ?\;H_2 \;(g)+ {\bf 1\;MgCl_2}\;(aq).

The number of \rm Mg and \rm Cl atoms shall be the same on both sides. Therefore

\rm {\bf 1\;Mg}\;(s) + {\bf 2\;HCl}\;(aq) \to ?\;H_2 \;(g)+ {1\;\underset{\wedge}{Mg}\underset{\wedge}{Cl_2}}\;(aq).

The number of \rm H atoms shall also conserve. Hence the equation:

\rm {1\;Mg}\;(s) + {2\;\underset{\wedge}{H}Cl}\;(aq) \to {\bf 1\;H_2 \;(g)}+ {1\;MgCl_2}\;(aq).

How many moles of HCl are available?

M(\rm HCl) = 1.008 + 35.45 = 36.458\;g\cdot mol^{-1}.

\displaystyle n({\rm HCl}) = \frac{m(\text{HCl})}{M(\text{HCl})} = \rm \frac{165.0\;g}{36.458\;g\cdot mol^{-1}} = 4.52576\;mol.

How many moles of Hydrogen gas will be produced?

Refer to the balanced chemical equation, the coefficient in front of \rm HCl is 2 while the coefficient in front of \rm H_2 is 1. In other words, it will take two moles of \rm HCl to produce one mole of \rm H_2. \rm 4.52576\;mol of \rm HCl will produce only one half as much \rm H_2.

Alternatively, consider the ratio between the coefficient in front of \rm H_2 and \rm HCl is:

\displaystyle \frac{n(\text{H}_2)}{n(\text{HCl})} = \frac{1}{2}.

\displaystyle n(\text{H}_2) = n(\text{HCl})\cdot \frac{n(\text{H}_2)}{n(\text{HCl})} = \frac{1}{2}\;n(\text{HCl}) = \rm \frac{1}{2}\times 4.52576\;mol = 2.26288\;mol.

What will be the volume of that many hydrogen gas?

One mole of an ideal gas occupies a volume of 22.4 liters under STP (where the pressure is 1 atm.) On certain textbook where STP is defined as \rm 1.00\times 10^{5}\;Pa, that volume will be 22.7 liters.

V(\text{H}_2) = \rm 2.26288\;mol\times 22.4\;L\cdot mol^{-1} = 50.69\; L, or

V(\text{H}_2) = \rm 2.26288\;mol\times 22.7\;L\cdot mol^{-1} = 51.37\; L.

The value "165.0 grams" from the question comes with four significant figures. Keep more significant figures than that in calculations. Round the final result to four significant figures.

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If there are 40 mol of NBr3 and 48 mol of NaOH, what is the excess reactant?
Nata [24]

Answer:

The correct answer is option B.

Explanation:

3NaOH+2NBr_3\rightarrow 3HOBr+3NaBr+N_2

Moles of NBr_3 = 40 mol

Moles of NaOH = 48 mol

According to reaction, 3 moles of NaOH reacts with 2 moles NBr_3

Then ,48 moles of NaOH will reacts with:

\frac{2}{3}\times 48 mol=32 mol of NBr_3

Then ,40 moles of NaBr_3 will reacts with:

\frac{3}{2}\times 40 mol=60 mol of NaOH

As we can see that 48 moles of sodium will completey react with 32 moles of nitrogen tribromide.

Moles left after reaction = 40 mol - 32 mol = 8 mol

Hence, the NBr_3 is an excessive reagent.

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How would i calculate molecules of water produced in a reaction?
levacccp [35]
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How many grams of CO 2 are present in a container with a volume of 5.61 L if the gas exhibits a pressure of 5.66 atm at a temper
Kruka [31]

Answer:

54.72 g

Explanation:

Mass = ?

Volume = 5.61 L

Pressure = 5.66 atm

Temperature = 311 K

The relationship between these equations is given by the ideal gas equation;

PV = nRT

where R = gas constant = 0.0821 atm L K-1 mol-1

n = PV / RT

n = 5.66 * 5.61 / (0.0821 * 311 )

n = 1.2436 mol

Number of moles = Mass / Molar mass

Mass = Number of moles * Molar mass = 1.2436 * 44 = 54.72 g

5 0
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