For a fixed mass of gasdk9eei .y9 uau2ot:r . at a constant temperature, what happens to the volume if the pressure of the gas eu iu. 2ko 9ar.:yetd9is doubled?

  Which of the following conditions makes gases deviate from idealhj.tnz2 (stj *967 t u9vgtxwp behavior?

  Based on the graph below, choose the correct statnc wl0szr37wpn( /;qa ement that describes the relationship between 7al c3/rqnw0psz(w;npressure and temperature for a fixed mass and volume of a gas?

  The ideal gas equation is a formula that combines the relationshipum9t*s+lmik x /k1b( t between pressure, volume, temperature, and the(/+9mbxmtluk*i1 t sk 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 1ky pr3j 96wsr;pxq4rcalculation to determine the final rrqp xs 94y3;pr jk16wvolume 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 inflated wit . igiqv6,wspi) yyx+4h $N_2$, 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 ga m hzz*rx ix(l7ou 1+93dktd1ds $(N_2)$ 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 cav j0z 1b:(i4dlwt; jddrs. The airbag is deployed as a b( d1i4;ldjzwd 0 vj:tsafety 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 aligns with the behaviorgx(t47 ;g e kasw6qp r532hvoq of an ideal ga5qrx6e3a 7h(kgt pvq;2g4sw os?

  Under which conditions would a gas deviate the most from the ideal gas model?4+artev *j 1-l.zmt ce

  A sample of gas at a certain temperature, pressure,ku 3gbkn cb.mzd wjop5fv 48q;e2y ;vniw485 ; 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 $T_2=\frac{1}{2}T_1$