Topic
Q:
\( \operatorname{MgBr}_{2} \)
\( \begin{array}{l}\text { acid } \\ \bigcirc \text { base } \\ \text { salt }\end{array} \)
Q:
Which best describes activation energy?A. the maximum amount of energy required to end a chemical reactionB. the amount of energy absorbed in an endothermic reactionC. the minimum amount of energy required to start a chemical reactionD. the amount of energy released in an exothermic reaction
Q:
When I drop blue dye into a beaker full of water the blue dye drop is extremely intense in
color at first, but the water eventually becomes a uniform lighter blue. How does this
scenario relate to diffusion?
Q:
Draw the Lewis structure of carbon monoxide \( (\mathrm{CO}) \) and then determine if the
molecule is polar or nonpolar. Please place the elements in the order that they are
written.
Q:
Draw the Lewis structure of \( \mathrm{CBr}_{4} \) and then determine its electron domain and
molecular geometries.
Q:
35 Metal \( X \) does not react with cold water but does react very slowly with steam
What is the position of \( X \) in the reactivity series?
A sodium \( \rightarrow X \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow \) copper
B sodium \( \rightarrow \) calcium \( \rightarrow X \rightarrow \) magnesium \( \rightarrow \) copper
C sodium \( \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow X \rightarrow \) copper
D sodium \( \rightarrow \) calcium \( \rightarrow \) magnesium \( \rightarrow \) copper \( \rightarrow X \)
Q:
Lattice enthalpy for NaCl is \( +788 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and
\( \Delta_{\mathrm{Hyd}}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1} \). Enthalpy of solution of \( \mathrm{NaCl}^{\circ} \) is
\( \begin{array}{ll}\text { (a) }+572 \mathrm{~kJ} \mathrm{~mol}^{-1} & \text { (b) }+4 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \text { (c) }-572 \mathrm{~kJ} \mathrm{~mol}^{-1} & \text { (d) }-4 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array} \)
Q:
A certain reaction is non spontancous at 298 K . The entropy
change during the reaction is \( 121 \mathrm{JK}^{-1} \). Is the reaction is
endothermic or exothermic? The minimum value of \( \Delta \mathrm{H} \) for
the reaction is
(a) endothermic, \( \Delta \mathrm{H}=36.06 \mathrm{~kJ} \)
(b) exothermic, \( \Delta \mathrm{H}=-36.06 \mathrm{~kJ} \)
(c) endothermic, \( \Delta \mathrm{H}=60.12 \mathrm{~kJ} \)
(d) exothermic, \( \Delta \mathrm{H}=-60.12 \mathrm{~kJ} \)
Q:
2 mole of an ideal gas at \( 27^{\circ} \mathrm{C} \) temperature is expanded
reversibly from 2 lit to 20 lit. Find the entropy change.
\( (R=2 \mathrm{cal} / \mathrm{mol} \mathrm{K}) \)
\( \begin{array}{llll}\text { (a) } 92.1 & \text { (b) } 0 & \text { (c) } 4 & \text { (d) }-9.2\end{array} \)
Q:
What is the entropy change (in \( \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \) ) when one
mole of ice is converted into water at \( 0^{\circ} \mathrm{C} \) ? (The enthalpy
change for the conversion of ice to liquid water is
\( 6.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \) at \( 0^{\circ} \mathrm{C} \) )
\( \begin{array}{llll}\text { (a) } 21.98 & \text { (b) } 20.13 & \text { (c) } 2.013 & \text { (d) } 2.198\end{array} \)
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