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UNO [17]
3 years ago
6

______ will have a higher entropy than 50.0 g CO2 (g) at 56 oC.

Chemistry
1 answer:
Tomtit [17]3 years ago
5 0
1) The more mass is the more entropy , because there are more particles, there is disorder.
2) Than higher temperature --- the more entropy.
3) Gas has more disorder than liquid, so gas has more entropy.
So, correct answer is E.
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A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 300.0 mL
Vera_Pavlovna [14]

Answer : The correct option is, (C) 1.7

Explanation :

First we have to calculate the moles of Ca(OH)_2 and HBr.

\text{Moles of }Ca(OH)_2=\text{Concentration of }Ca(OH)_2\times \text{Volume of solution}=0.10M\times 0.1L=0.01mole

\text{Moles of }HBr=\text{Concentration of }HBr\times \text{Volume of solution}=0.10M\times 0.3L=0.03mole

The balanced chemical reaction will be:

Ca(OH)_2+2HBr\rightleftharpoons CaBr_2+2H_2O

0.01 mole of Ca(OH)_2 dissociate to give 0.01 mole of Ca^{2+} ion and 0.02 mole of OH^- ion

and

0.03 mole of HBr dissociate to give 0.03 mole of H^+ ion and 0.03 mole of Br^- ion

That means,

0.02 moles of OH^- ion  neutralize by 0.02 moles of H^+ ion.

The excess moles of H^+ ion = 0.03 - 0.02 = 0.01 mole

Total volume of solution = 100 + 300 = 400 ml = 0.4 L

Now we have to calculate the concentration of H^+ ion.

\text{Concentration of }H^+=\frac{\text{Moles of }H^+}{\text{Total volume}}

\text{Concentration of }H^+=\frac{0.01mole}{0.4L}=0.025M

Now we have to calculate the pH of the solution.

pH=-\log [H^+]

pH=-\log (0.025M)

pH=1.7

Therefore, the pH of the solution is, 1.7

5 0
3 years ago
In the first half of the Citric acid cycle, ____________ is oxidized, yielding a pair of electrons that reduce a molecule of NAD
KiRa [710]

Answer:

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Explanation:

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ivann1987 [24]

false

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3 0
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andre [41]
Lead-
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bazaltina [42]
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</span>
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