For a fixed mass of gas at a con328ukhp3c lgh57qtk a stant temperature, what happens to the volume if the pr ta5873g3kcq ukh2plhessure of the gas is doubled?

  Which of the followinahpp ;krog 7 j u)2nal5dg3au /;bsy)2g conditions makes gases deviate from ideal behavior?

  Based on the graph below,ezaka5s:91jz6.da8v /fb as uh c 28dz choose the correct statement that describes the relationship between pressure and temperature for a fixed mass and volu az 8bessj9z.c 2k: hva15u f8a6d/zadme of a gas?

  The ideal gas equation is a formula that combines the relat l3w mdl 3xz,uf6p)hx*ionship between pressurp3z *uw fl36xmhl) ,dxe, 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 correc1)pma yd6 l+hp ml;py.t calculation to determine the final volume of a fixed masy6 ;yl 1.p hmm)+lppdas 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 witi f:+ohql*e6q xxerzf (/1kt/h $N_2$, 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 g7md1m l .eq x7ri7fcy4as $(N_2)$ 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 wevf25c1hn qhp38 )b z b+ fgf(v5x/fuuithin the airbags of some older cars. The airbag is deployed as a safetnu5ef)f bf3 zx( ghfu2v+ /q5b8 c1hpvy feature 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 gases most closely a41 slz+l4 kc0x pr8shgo1 e9stligns with the behavior of an ideal gas?81c9k 0 ogs s l1ps4rz+hxlt4e

  Under which conditions would a gas deviate the most from the ideal gc n 79(vw(9ps1giok:4f:bofl 6txqy l as model?

  A sample of gas at aw(yd h:qihe/t:2, go b certain temperature, 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 $T_2=\frac{1}{2}T_1$