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Maksim231197 [3]
3 years ago
12

Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?A) This reaction will be

spontaneous only at high temperatures.B) This reaction will be spontaneous at all temperatures.C) This reaction will be nonspontaneous at all temperatures.D) This reaction will be nonspontaneous only at high temperatures.E) It is not possible to determine without more information.
Chemistry
1 answer:
Alja [10]3 years ago
4 0

Answer: A) This reaction will be spontaneous only at high temperatures

Explanation:

\Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

Using Gibbs Helmholtz equation:

\Delta G=\Delta H-T\Delta S

Given : \Delta H=+ve

\Delta S=+ve

\Delta G=(+ve)-T(+ve)

\Delta G=(+ve)(-ve)

Thus the value of  \Delta G  is negative and spontaneous when temperature is high.

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What mass of solute must be used to prepare 500ml of 0.100M aqueous sodium borate Na2B4O7 from solid hydrated sodium borate Na2B
motikmotik

0.000132 g of hydrated sodium borate (Na₂B₄O₇ · 10 H₂O)

Explanation:

First we need to find the number of moles of sodium borate (Na₂B₄O₇) in the solution:

molar concentration = number of moles / volume (L)

number of moles = molar concentration × volume (L)

number of moles of Na₂B₄O₇ = 0.1 × 0.5 = 0.05 moles

We know now that we need 0.05 moles of hydrated sodium borate (Na₂B₄O₇ · 10 H₂O) to make the solution.

Now to find the mass of hydrated sodium borate we use the following formula:

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mass of hydrated sodium borate = 0.05 / 381 = 0.000132 g

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