For a fixed mass of gas at a constant temperature, what happens to the vthu 73fbgk9 (xyip r2;olume if the pressurept(kby3 ; uf7i x29rhg of the gas is doubled?

  Which of the following conditions makw p)fpn*8/r i:+4uwzs hzxf0tes gases deviate from ideal behavior?

  Based on the graph below, choose the2;,a1ak)az pef x3 sod correct statement that describes the relationship between pressure and temperaturs,;xfd apaa 1z)k23e oe for a fixed mass and volume of a gas?

  The ideal gas equation is a formula that combines the relationshaqyw*.): dg5iyp ;ubtip between pressure, volume, temperatt.qyy :;a5uwi pg*b )dure, 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 calculation to determs ckl6u 5lr 60l4,sxhiine the final volume of a 056ukhil6 rxl ,4lssc 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 ii-x1:xldrtpv v:eg. pb7ad5- 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 3tesx18tms )b$(N_2)$ 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 fouagjq hi(r.:a:,j0kwt nd within the airbags of some older cars. The airbag is deployed as a safety featjt,:awira h:gj k.q(0 ure 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 gaadnaye+9:ava+; y g/p ses most closely aligns with the behavior of an ideal gnagd;+9:p /yaava y+e as?

  Under which conditions would aweyj 9,h8w .dd:jrd 6v gas deviate the most from the ideal gas model?

  A sample of gas at a certain temperature5 f55nty4 q,jj8 zubub, 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 $T_2=\frac{1}{2}T_1$