For a fixed mass of gas at a constant temperature, what happens vhszipm /vb 2)vwtj2 tg*)3i/to the volume if the pressure of th bvzv)/ mjti3ihw2v )gt2*s /pe gas is doubled?

  Which of the following condpujg4v 9e5 a4 )4ranldu7g x0qitions makes gases deviate from ideal behavior?

  Based on the graph below, choose the correct(.amxx(k(0,lgu 4rk jp+n gei statement that describes the relationship between pressure and temp lxj((agim.e+4x(k g,0ru npkerature for a fixed mass and volume of a gas?

  The ideal gas equation is a formula t0:z hd3du 4mrd s4h:uk;mxxq3hat combines the relationship between pressux d:m; mu 3h4rk4 3dhs0xd:quzre, volume, temperature, and the number 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 below, what is the correct calccz* gp(fh:;+xn2o kaxulation to determine the final vo+2 p *gxfoh(;zx:ncka lume of a fixed 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 i) zu)6dd9n -ds9dxppd nflated with $N_2$, 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 gas bfb04:tb a 8tm1ph j2o$(N_2)$ 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 some older ca, eto(,uj6 iegrs. The airbag is deployed as a safety feai,e,jt(g 6u eoture in the event of an accident. In this application, 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 guj:f 2 (lkci5pases most closely aligns with the behavior of an ideal ga:fpij lu2ck5(s?

  Under which conditions would a gas dev0fnh*xvy -ia10hkvw2 iate the most from the ideal gas model?

  A sample of gas at a certain temperature, :ab 2jsohddw+su6qg. 6 o x5y8pressure, and 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 $T_2=\frac{1}{2}T_1$