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boyakko [2]
1 year ago
10

Which statement about spontaneous and nonspontaneous processes is correct? Spontaneous processes are favored by a decrease in De

lta. H, but nonspontaneous reactions are favored by an increase in Delta. H. Spontaneous processes are favored by a decrease in Delta. S, but nonspontaneous reactions are favored by an increase in Delta. S. An increase in Delta. S favors both spontaneous and nonspontaneous processes. A decrease in Delta. H favors both spontaneous and nonspontaneous processes.
Chemistry
1 answer:
cupoosta [38]1 year ago
6 0

The statement correct for the processes are spontaneous reaction have negative Delta H and non-spontaneous reaction has positive Delta H. Hence, option A is correct.

The value of Delta H in the reaction is the change in enthalpy of the reaction. The enthalpy of the reaction determines the reaction to be spontaneous or non-spontaneous.

<h3>What determines spontaneous and non-spontaneous reaction?</h3>

The spontaneous reaction is required with the energy input for the reaction to proceed. The energy is required by the system thus, the value of Delta H is negative.

The non-spontaneous reaction requires with the loss of energy in the formation of the product. The energy released gives the values of Delta H positive.

Thus, the statement correct for the processes are spontaneous reaction have negative Delta H and non-spontaneous reaction has positive Delta H. Hence, option A is correct.

Learn more about Delta H, here:

brainly.com/question/10601562

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Silver nitrate reacts with aluminum chloride to form the insoluble compound, silver chloride. The reaction proceeds according to
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The theoretical yield of silver chloride, AgCl is 5.2109 g

The balanced equation for the reaction is given below:

<h3>3AgNO₃(aq) + AICI₃(aq) —> Al(NO₃)₃ (aq) + 3AgCl (s) </h3>

Next, we shall determine the mass of aluminum chloride, AICI₃ that reacted and the mass of silver chloride, AgCl produced from the balanced equation. This is illustrated below:

Molar mass of AICI₃ = 133.34 g/mol

Mass of AICI₃ from the balanced equation = 1 × 133.34 = 133.34 g

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<h3>SUMMARY</h3>

From the balanced equation above,

133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.

Finally, we shall determine the theoretical yield of AgCl by the reaction of 1.616 g of AICI₃ as follow:

From the balanced equation above,

133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.

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1.616 g of AICI₃ will react to produce = \frac{1.616 * 429.96}{133.34} = 5.2109 g of AgCl.

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