For a fixed mass of gas at a constant temperaur1lz ak-2 c d9nnkeau9qb/69ture, what happens to the volume if the a2uqkna k rz9-96n/ud1 lc9be pressure of the gas is doubled?

  Which of the following conditions makes gases deviate from ideal behrqfvl5 jq z,*: q(,skzavior?

  Based on the graph below, choose the correct statementzf2gkm jq22uep8)4qq that describes the relationship between pressure and temperature for a fixed mass and volumq)fk q22ge 2jqp8m4uze of a gas?

  The ideal gas equation is a formula that combines the relationship between pmgu ;vl6ix y;adbz: w6nx*. :rressure, volume, temperatubry;wlm xduz: gnx6:a;. *i 6vre, 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 c2l 7whzigjye+exk 0 +6xuk. ;worrect calculation to determine the final vuxi+yh.2;6 w0xee j7klzkg+ w olume 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 infle;7p*y//m rf ts:pg4: twaxvhated 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 f d(gr,g8kj0k:rfd+/,poc: xp6jl y u$(N_2)$ 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 4,o m3re6wver cars. The airbag is deployed as a safety feature in the event of an accident. In this application, the sodium azide decomposes3 ,emvrr oe4w6 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 clomt +2);evsnl 5r4dq ygsely aligns with the behavior of an ideal gas?qg5; )42vrlm ste+yn d

  Under which conditions would a gas deu mibl*.z1)o iviate the most from the ideal gas model?

  A sample of gas at a certain temperature, pressure, an d(q9 inuribu 5m/z3y:hdc -2p)/h vgcd 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 $T_2=\frac{1}{2}T_1$