For a fixed mass of gas at a constant tempeu 0pei le5i.9lrature, what happens to the volume if the pressure of the gas is pl.euiil 509 edoubled?

  Which of the following conditions makes gaseg,5ut iwp7w)/m*qqiejc p8k ,s deviate from ideal behavior?

  Based on the graph below, choose the correct statement that des68pl,,m pc.z 89sgsovhmipa 6q pyj6*cribes the relationship between pressure and temperature for a fih6qc86mo,pzl*mgipps8j ,a9.syv6 pxed mass and volume of a gas?

  The ideal gas equation is a .q3b qxkyok6) formula that combines the relationship between pressure, volume, temperature, and the y3) qx6b qo.kknumber of moles.
1.Complete the table below by calculating the missing variables of the ideal gas equation.

P	V	n	T
$\times10^4$Pa	$0.015m^3$	0.400mol	$37^{\circ}C$
152,000Pa	$m^3$	2.00mol	298.15K
31,000Pa	$0.25m^3$	mol	271.15K
250kPa	$0.75dm^3$	0.580m0l	k

2.A $256cm^3$ flask contains 0.800g of a gaseous compound with an empirical formula of CHCl. The pressure and the temperature of the gas are respectively $10^5$, Pa10 and 373K. Determine the molecular formula of the compound.

  Liquid butanol $(C_4H_9OH)$ burns or combusts in oxygen to produce $CO_{2(g)}$ and $H_2O$(g).
1.Write a balanced equation, including state symbols, for this reaction.
2.When $1.250cm^3$ of butanol is combusted in excess oxygen,$1.921dm^3$ of water vapor is collected at a pressure of 125.0 kPa and $150.0^{\circ}C$. Calculate the moles of butanol that were combusted.  mol
3.Determine the density of liquid butanol in $g\:cm^{-3}$.  g $cm^{-3}$

  Based on the table belon)7e1jqprw8nv :akeoo1 58hiw, what is the correct calculation to determine the final volume of a fi 1 nirvhj5o1a8:k7qenwope)8 xed mass of gas:

Initial	Final
Pressure = 1.00 atm	Pressure = 1.60 atm
Temperature =$20^{\circ}C$	Temperature =$10^{\circ}C$
Volume =$5.00dm^3$	Volume = ?

  Automobile airbags are inflated with s+ fx0( k2f. cyjh pvh10ru*mu$N_2$, a byproduct of sodium azide decomposition, according to the following reaction.
$2NaN_{3(s)}\rightarrow2 Na_{(s)}+3N^{2(g)}$
Calculate the mass (in grams) of sodium azide needed to generate $0.07m^3$ of $N^2$ at $1.01\times10^{5}Pa$ and $26.0^{\circ}C$.$n_{N2}$=  mol, mass of $NaN_3$=  g

  14.01g of nitrogen gaie5 uo x*q)ea8c0a.4 uw0sa1f *fb dzus $(N_2)$ is reacted with excess $H_2$. What volume of ammonia $(NH_3)$gas would be produced at STP? The molar volume of a gas at STP is $22.7dm^3$.
$N_{2(g)}+3H_{2(g)}\rightarrow2NH_{3(g)}$

  Sodium azide is an ionic compound found within the airbags of sb5oev)pyj 6+r ome older cars. The airbag is deployed as a safety feature in the event of an accident. In this applica5e+vj6) obp yrtion, the sodium azide decomposes rapidly, and the gas formed inflates the airbag.
The decomposition of sodium azide under these conditions is given below.
$2NaN_{3(s)}\rightarrow2Na (s)+3 N_{2(g)}$
1.Suggest the formula and charge for the azide ion.
2.A typical airbag requires $65.0dm^3$of nitrogen gas for complete inflation at STP. Using section 2 of the data booklet, calculate the mass of sodium azide that the airbag must contain for this purpose.Molar mass for sodium azide calculated=  $g mol^{-1}$

  Which of the following gases most closely aligns with the behavior of ang;xi t:1li.z * 5oy 1scf1dvd1ha-cnm,5kf t j ideal gvk1:ta xm5lcfs,ji*. gt zco;hi51 -1ddfyn 1as?

  Under which conditions would a gas deviate5b: ahaqaoj+* vu9 ,rj the most from the ideal gas model?

  A sample of gas at a certain temperature, pressure, and s 79u u,(j+hup*+bm/lfv ndyu volume $(T_1,P_1,and V_1T)$ undergoes a change in temperature and pressure $(T_2andP_2)$.What is the new volume $(V_2)$?
Before: $T_1,P_1,V_1$;
After: $P_2=2P_1$ AND $T_2=\frac{1}{2}T_1$