Question $1.$ At a temperature of $311$ K$,\_\_\_\_\_$

moles of an ideal gas occupy $962\mathrm{.}9$ mL at $774\mathrm{.}3$ mm Hg$.$ Question $2.$ The density of ammonia gas, NH$3,$ in a $4\mathrm{.}52$ L container at $957$ torr and $30\mathrm{.}2$oC is $\_\_\_\_\_$

g$/$L$.$ Question $3.$ A gas sample originally was held at a volume of $5\mathrm{.}98$ L at $44\mathrm{.}2$ oC and a pressure of $707$ torr. In order to reduce its volume to $2\mathrm{.}23$ L$,$ at constant pressure, this gas must be cooled to $\_\_\_\_\_\_$oC$.$ Question $4.$ The volume of $0\mathrm{.}798$ moles of an ideal gas at $586$ torr and $23\mathrm{.}8$ oC is $\_\_\_\_\_$ L$.$ Question $5.$ The pressure in a $13\mathrm{.}3$ L vessel that contains $4\mathrm{.}73$ g of carbon dioxide, $4\mathrm{.}02$ g of sulfur dioxide and $4\mathrm{.}49$ g of argon, all at $50\mathrm{.}4$ oC is $\_\_\_\_\_$mmHg$.$ Question $6.$ A gas sample is attached to an open$-$ended mercury manometer, as shown below. The difference in heights of the mercury in the manometer is $15\mathrm{.}9$ cm when the atmospheric pressure is $691$ torr. Given that the density of mercury is $13\mathrm{.}6$ g$/$mL$,$ the pressure of the enclosed gas is $\_\_\_\_\_\_\_$atm. Question $7.$ A $2\mathrm{.}66$ gram sample of helium gas exhibits a pressure of $2\mathrm{.}33$ atm in a $7\mathrm{.}17$ L volume. The sample is compressed to a $3\mathrm{.}77$ L volume at constant temperature. After the compression, the gas pressure is $\_\_\_\_\_\_$atm. Question $8.$ A gas mixture contains only Ne and Ar$,$ has a total pressure of $3\mathrm{.}54$ atm, and contains $12\mathrm{.}6$ mol of gas. If the partial pressure of Ne is $2\mathrm{.}88$ atm, how many moles of Ar are in the mixture? Question $9.$The molar mass of a gas is $\_\_\_\_\_\_$

g$/$mol if $7\mathrm{.}466$ g of the gas occupies $4\mathrm{.}462$ L at a temperature of $421\mathrm{.}5$ K and $734\mathrm{.}7$ torr pressure. Question $10.$Hydrogen gas is produced from the reaction of Zn$($s$)$ with sulfuric acid, based on the following equation.

Zn $($s$)+$ H$2$SO$4($aq$)->$ ZnSO$4($aq$)+$ H$2($g$)$

A sample of Zn$($s$)$ was mixed with excess H$2$SO$4($aq$)$ and the resulting H$2$ gas was collected over water. $0\mathrm{.}691$ liters of wet H$2($g$)$ were collected at $23\mathrm{.}6$ oC when the atmospheric pressure was $699$ mmHg$.$ Based on this information, $\_\_\_\_\_\_\_\_\_$

grams of Zn$($s$)$ were consumed during the process. The vapor pressure of water at this temperature is $26$ mmHg$.$ Question $11.$ Sodium hydride reacts with water to produce sodium hydroxide and hydrogen gas:

NaH $($s$)+$ H$2$O $($l$)->$ NaOH $($aq$)+$ H$2($g$)$

A sample of NaH weighing $\_\_\_\_\_\_$

g will produce $382$ mL of dry hydrogen gas at $29\mathrm{.}3$ oC and $736$ torr, when reacted with a stoichiometric quantity of water.