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Mamont248 [21]
3 years ago
12

A solution is prepared by adding 0.0231moles of H3O+ ions to 3.33L of water. What is the pH of this solution

Chemistry
1 answer:
MrMuchimi3 years ago
8 0

Answer:

2.15

Explanation:

For this question, we have to remember the <u>pH formula</u>:

pH~=~-Log[H_3O^+]

By definition, the pH value is calculated when we do the -Log of the concentration of the <u>hydronium ions</u> (H_3O^+). So, the next step is the calculation of the <u>concentration</u> of the hydronium ions. For this, we have to use the <u>molarity formula</u>:

M=\frac{mol}{L}

We already know the number of moles (0.0231 moles) and the volume (3.33 L). So, we can plug the values into the molarity formula:

M=\frac{0.0231~moles}{3.33~L}=0.00693~M

With this value, now we can calculate the pH value:

pH~=~-Log[0.00693~M]~=~2.15

<u>The pH would be 2.15</u>

I hope it helps!

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Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by the following reaction: C(s)+2H2O(g)→2H2
madam [21]

The question is incomplete , complete question is:

Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by the following reaction:

C(s)+ 2 H_2O(g)\rightarrow 2H_2(g)+CO_2(g).\Delta H=?

Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate ΔH of reaction for this reaction.

Answer:

The ΔH of the reaction is -626 kJ/mol.

Explanation:

C(s)+ 2 H_2O(g)\rightarrow 2H_2(g)+CO_2(g).\Delta H=?

We are given with:

\Delta H_{H-O}=459 kJ/mol

\Delta H_{H-H}=432 kJ/mol

\Delta H_{C=O}=799 kJ/mol

ΔH =  (Energies required to break bonds on reactant side) - (Energies released on formation of bonds on product side)

\Delta H=(4\times \Delta H_{O-H})-(2\times \Delta H_{H-H}+2\times\Delta H_{C=O})

=(4\times 459 kJ/mol)-(2\times 432 kJ/mol+2\times 799 kJ/mol

\Delta H=-626 kJ/mol

The ΔH of the reaction is -626 kJ/mol.

5 0
3 years ago
Calculate the number of moles of O2 gas held in a sealed 2.00 L tank at 3.50 atm and 25 ℃.
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Answer:

n=0.286mol

Explanation:

Hello,

In this case, we consider oxygen as an ideal gas, for that reason, we use yhe ideal gas equation to compute the moles based on:

PV=nRT\\\\n=\frac{PV}{RT}

Hence, at 3.50 atm and 25 °C for a volume of 2.00 L we compute the moles considering absolute temperature in Kelvins:

n=\frac{3.50atm*2.00L}{0.082\frac{atm*L}{mol*K}(25+273)K} \\\\n=0.286mol

Best regards.

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Answer:

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Explanation:

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