For a fixed mass of gas at a constant temperature, what happen(widb64cu q7*mj t qn*s to the volume if the press* 6bmd7uqi4t( nj*wc qure of the gas is doubled?

  Which of the following conditions makes7hcb7nt jv19x gases deviate from ideal behavior?

  Based on the graph below, choose the correct statement that describes the rh+hs 06t tka8, tjv1mkelationship between pressure and temperature for a fixedk0tt6hh8vatj k +1m,s mass and volume of a gas?

  The ideal gas equation ic/r3(9wvg0l;g,9o ehtcl f q us a formula that combines the relationship between pressure, volume, temperature, and the 9gr/c ,0tq ;wve3 fcoh9llu(gnumber 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 calw )ll;wmurhi tb;wzpg21 we397)5um gculation to determine the final volume of a fixed mass2wz );wue 3g 7)gwwbprml9 1tmu;5ilh 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 yh togdfih/ ;o i7*v bqp-+v-6with $N_2$, 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 ganb5 ft o:89,i-6qs kc3 ,tw mjj,pahlis $(N_2)$ 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 aii. *3du6pqsv zc9 4nckrbags of some older cars. The airbag is deployed as a safety feature in the event of an accident. In this application, the sodium azide decomposes rapidly, and the gas formed inflates the*s 6ic43du.qp cvz9nk 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 gavqms1mu4k-0 t k z*-twses most closely aligns with the behavior of an ideal gas?q1tukkvw-m0m t*z- s 4

  Under which conditions would a gas deviate the most vglph.c -4zgldv 6.) luf/.czfrom the ideal gas model?

  A sample of gas at a certain tempep5: ,r ftnqlq;rature, pressure, 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 $T_2=\frac{1}{2}T_1$