Find the enthaipy change, $M,$ for the following reaction using the information in the rable below:

$($A$)-544k\frac{J}{m}ol$

$($B$)+544k\frac{J}{m}ol$

$($C$)+21k\frac{J}{m}ol$

$($D$)-21k\frac{J}{m}ol$

$($E$)+1151k\frac{J}{m}ol$

For a given process at constant pressure, $w$ is positive. This means that the process involves

A$)$ work being done by the system on the surroundings

$($B$)$ work being done by the surroundings on the system

C$)$ no work being done

D$)$ an equal amount of work done on the system and by the system

E$)$ work being done against a vacuum

For a particular process $q=-17kJ$ and $w=21kJ.$ Which of the following statements is false?

A$)$ Heat flows from the system to the surroundings.

B$)$ The system does work on the surroundings.

C$)E=+4kJ$

D$)$ The process is exothermic.

E$)$ None of the above is false.

Calculate the work associated with the expansion of a gas from $42\mathrm{.}0L$ to $79\mathrm{.}0L$ at a constant pressure of $14\mathrm{.}0$atm.

A$)518L*atm$

B$)-518L*atm$

C$)-1\mathrm{.}11{10}^{3}L*atm$

D$)588L*atm$

E$)1\mathrm{.}11{10}^{3}L*atm$

What is the specific heat capacity of a metal if it requires $169\mathrm{.}6J$ to change the temperature of $15\mathrm{.}0g$ of the metal from $25\mathrm{.}00C$ to $32\mathrm{.}00C?$

A$),0\mathrm{.}619\frac{J}{g}C$

B$),11\mathrm{.}3\frac{J}{g}C$

C$),24\mathrm{.}2\frac{J}{g}C$

$($D$)1\mathrm{.}62\frac{J}{g}C$

E$),275\frac{J}{g}C$

Consider the reaction:

$q=mcT$

$T_f-T_{\text{I}}$

$(32-25)$

$169\mathrm{.}6J=15\mathrm{.}0g(x)!in7$

${?}_{2x}{C}_2{H}_{5}OH(l)+3O_2(g)2C{O}_2(g)+3H_{2}O(l),H=-1\mathrm{.}37{10}^{3}kJ$

When a $27\mathrm{.}8-$g sample of ethyl alcohol $($molar mass $=46\mathrm{.}07\frac{g}{m}ol)$ is burned, how much energy is released as heat?

A$)0\mathrm{.}603kJ$

B$)0\mathrm{.}827kJ$

C$)8\mathrm{.}27{10}^{2}kJ$

D$)3\mathrm{.}81{10}^{4}kJ$

E$)1\mathrm{.}66kJ$

The $H$ value for the reaction is $-90\mathrm{.}8kJ.$ How much heat is released when $88\mathrm{.}1gHg$ is reacted with oxygen?

A$)0\mathrm{.}439kJ$

B$)8\mathrm{.}00103kJ$

C$)39\mathrm{.}9kJ$

D$)90\mathrm{.}8kJ$

E$)$ none of these

$C{H}_4(g)+4C{l}_2(g)CC{l}_4(g)+4HCl(g),H=-434kJ$

Based on the above reaction, what energy change occurs when $1\mathrm{.}2$ moles of methane $(C{H}_4)$ reacts?

A$)5\mathrm{.}2{10}^{5}J$ are released.

B$)5\mathrm{.}2{10}^{5}J$ are absorbed$.$

C$)3\mathrm{.}6{10}^{5}J$ are released.

D$)3\mathrm{.}6{10}^{5}J$ are absorbed$.$

E$),4\mathrm{.}4{10}^{5}J$ are released.