Consider the following reaction

Which of the following would increase the value of $K?$

a$.$ Increase $H$

b$.$ Increase pressure

c$.$ Decrease $[$C$]$

d$.$ Decrease pressure

e$.$ Decrease temperature

$2.$ Which of the following conditions always results in an increase in the internal energy $(AE>0$ of a system?

a$.$The system gains heat and has work done on it by the surroundings.

b$.$The system gains heat and does work on the surroundings.

c$.$ The system loses heat and does work on the surroundings.

d$.$ The system loses heat and has work done on it by the surroundings.

e$.$ None of them.

$3.$ The following reaction obeys the rate law; Rate $=k[N_2{O}_5{]}^2$ with a rate constant of $0\mathrm{.}139M^{-1}{s}^{-1}.$ If a reaction vessel contains $0\mathrm{.}620M{N}_2{O}_5$ initially, calculate the concentration of $N_2{O}_5$ in the vessel $220$ seconds after the reaction has begun.

$2N_2{O}_5(g)2N_2{O}_4(g)+O_2(g)$

a$.1\mathrm{.}183M$

b$.0\mathrm{.}00032M$

c$.0\mathrm{.}84M$

d$.0\mathrm{.}0311M$

e$.0\mathrm{.}053M$

$4.?$

$5.$ Graphite $($a form of solid carbon$)$ is added to a vessel that contains pure $C{O}_2(g)$ at a pressure of $0\mathrm{.}824$atm at a certain high temperature. The pressure in the vessel rises to an equilibrium value of $1\mathrm{.}366$atm as a single reaction occurs to produce CO $(g)$ and no other products. Determine the value of its corresponding equilibrium constant.

$C(s,$ graphite $)+C{O}_2(g)2CO$

$($g$)$

a$.3\mathrm{.}84$

b$.0\mathrm{.}26$

c$.4\mathrm{.}210-2$

d$.4\mathrm{.}17$

e$.1\mathrm{.}03101$