Topic
Q:
Calculate the cell potential for the galvanic cell in which the given reaction occurs at \( 25^{\circ} \mathrm{C} \), given that \( \left[\mathrm{Sn}^{2+}\right]=0.0673 \mathrm{M} \),
\( \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Co}^{3+}(\mathrm{aq}) \rightleftharpoons \mathrm{Sn}^{4+}(\mathrm{aq})+2 \mathrm{Co}^{2+}(\mathrm{aq}) \)
Q:
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at \( 25^{\circ} \mathrm{C} \).
\[ \mathrm{Pt}(\mathrm{s})\left|\mathrm{Sn}^{2+}(0.0062 \mathrm{M}), \mathrm{Sn}^{4+}(0.11 \mathrm{M}) \| \mathrm{Fe}^{3+}(0.11 \mathrm{M}), \mathrm{Fe}^{2+}(0.0018 \mathrm{M})\right| \mathrm{Pt}(\mathrm{s}) \]
\( E_{\mathrm{Sn}^{4+} / \mathrm{Sn}^{2+}}^{\circ}=0.154 \mathrm{~V} \quad E_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=0.771 \mathrm{~V} \)
Q:
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at \( 25^{\circ} \mathrm{C} \).
\( \begin{array}{l}\mathrm{Cu}(\mathrm{s})\left|\mathrm{Cu}^{2+}(0.13 \mathrm{M}) \| \mathrm{Fe}^{2+}(0.0017 \mathrm{M})\right| \mathrm{Fe}(\mathrm{s}) \\ E_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\circ}=0.339 \mathrm{~V} \quad E_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\circ}=-0.440 \mathrm{~V}\end{array} \)
Q:
What is the mass in grams of a sample of water when the temperature drops
from \( 75.00^{\circ} \mathrm{C} \) to \( 56.00^{\circ} \mathrm{C} \) and 800.0 J of energy are lost?
- Enter the answer with four significant figures.
- Use \( 4.184 \frac{\mathrm{~J}}{\mathrm{~g}^{\circ} \mathrm{C}} \) for the specific heat of water.
Provide your answer below:
Q:
Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations.
\[ \mathrm{Sn}(\mathrm{s})\left|\mathrm{Sn}^{2+}(\mathrm{aq}, 0.0155 \mathrm{M}) \| \mathrm{Ag}^{+}(\mathrm{aq}, 1.50 \mathrm{M})\right| \mathrm{Ag}(\mathrm{s}) \]
net cell equation: \( \mathrm{Sn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s}) \)
Calculate \( E_{\text {cell }}^{\circ} \) and \( E_{\text {cell }} \) at \( 25^{\circ} \mathrm{C} \), using standard potentials as needed.
Q:
An unknown metal at \( 100.0^{\circ} \mathrm{C} \) with specific heat \( 1.14 \frac{\mathrm{~J}}{\mathrm{~g}^{\circ} \mathrm{C}} \) is placed in \( 750 . \mathrm{g} \) of
water at \( 25.0^{\circ} \mathrm{C} \). The final temperature of the water is \( 28.6^{\circ} \mathrm{C} \). What was the
mass of the metal?
- Round your answer to the nearest integer.
- Use \( 4.184 \frac{\mathrm{~J}}{\mathrm{~g}^{\circ} \mathrm{C}} \) for the specific heat of water.
Provide your answer below:
Q:
Question
30. g of an unknown substance at \( 120.0^{\circ} \mathrm{C} \) is placed in 600.0 g of water at
\( 30.0^{\circ} \mathrm{C} \). The final temperature of the water is \( 31.4^{\circ} \mathrm{C} \). What was the specific heat
of the metal?
- Round your answer to one decimal place
- Use \( 4.184 \frac{\mathrm{~J}}{\mathrm{~g} \mathrm{C}} \) for the specific heat of water.
Provide your answer below:
line
Q:
Which of the following salts is water soluble?
\( \begin{array}{l}\text { KClO3 } \\ \text { O BaSO4 } \\ \text { O } \\ \mathrm{Ag3PO} 4 \\ \mathrm{FeCO} 3\end{array} \)
Q:
Which one of the following is a strong acid?
HF
HNO 2
HBrO
HCN
HI
Q:
Which one of the following is NOT a soluble base?
\( \begin{array}{l}\mathrm{O} \mathrm{CsOH} \\ \mathrm{KOH} \\ O \mathrm{Fe}(\mathrm{OH}) 2 \\ \mathrm{Ca}(\mathrm{OH}) 2 \\ \mathrm{Oa}(\mathrm{OH}) 2\end{array} \)
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