Consider the reaction below: A_{(aq)} ? B_{(aq)} quad Delta G^{o}_{rxn} = -2.01 kJ A 1.000 M solution of A was heated at 65.9 °C for several hours. After some time the concentration of A was determined. Answer the following questions: a) What is the maximum amount of work (?G) from/for this reaction when [A] = 0.824 M? ?G_{(kJ)} = b) What is the concentration of B when ?G = -2.56 kJ? [B]_{M} = c) Determine Q when ?G = -6.06 kJ? Q =
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$$ \begin{aligned} &\text { Calculate the value of } \Delta G \text { at } 700 \mathrm{~K} \text { for the reaction } n X \longrightarrow m B .^{-1}\\ &\text { Given that value of } \Delta H=-113 \mathrm{~kJ} \mathrm{~mol}^{-1} \text { and } \Delta S=-145 \mathrm{JK} \mathrm{mol}^{-1} \text { . } \end{aligned} $$
Given the values of $\Delta H_{\mathrm{rm}}^{\circ}, \Delta S_{\mathrm{rm}}^{\circ},$ and $T,$ determine $\Delta S_{\mathrm{univ}}$ and predictwhether each reaction is spontaneous. $ a.\quad \Delta H_{\mathrm{rxn}}^{\circ}=+115 \mathrm{k} J ; \quad \Delta S_{\mathrm{mn}}^{\circ}=-263 \mathrm{J} \quad {K} T=298 \mathrm{K} $ $ b.\quad \Delta H_{\mathrm{rxn}}^{\circ}= - 115 \mathrm{k} J ; \quad \Delta S_{\mathrm{mn}}^{\circ}=+263 \mathrm{J} \quad {K} T=298 \mathrm{K} $ $ c.\quad \Delta H_{\mathrm{rxn}}^{\circ}= - 115 \mathrm{k} J ; \quad \Delta S_{\mathrm{mn}}^{\circ}=-263 \mathrm{J} \quad {K} T=298 \mathrm{K} $ $ c.\quad \Delta H_{\mathrm{rxn}}^{\circ}= - 115 \mathrm{k} J ; \quad \Delta S_{\mathrm{mn}}^{\circ}=-263 \mathrm{J} \quad {K} T=615 \mathrm{K} $
The rate of a certain reaction was studied at various temperatures. The table shows temperature (𝑇) ( T ) and rate constant (𝑘) ( k ) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, 𝐸a E a , for this reaction? 𝑇 (𝐊) T ( K ) 𝑘 (𝐬−1) k ( s − 1 ) 400 400 0.000105 0.000105 420 420 0.000658 0.000658 440 440 0.00348 0.00348 460 460 0.0159 0.0159 480 480 0.0643 0.0643 500 500 0.232 0.232 520 520 0.758 0.758 540 540 2.27 2.27 560 560 6.29 6.29 580 580 16.2 16.2 𝐸a= E a = kJ⋅mol−1 kJ ⋅ mol − 1 What is the value of the pre‑exponential factor (sometimes called the frequency factor), 𝐴 A , for this reaction? 𝐴= A =
David C.
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