For a fixed mass of gas at a constant temperature, wh 2*5l8vo8gwn7s;ij6h1f ch4gn avo js at happens to the volume if the pressure of the gas is doubleh28ijh6ga j7 wvv4c1o*nf o l 8gs;s5nd?

  Which of the following conditions makes gassts lr7vuoy +8m9wc.j2c)gw 5 es deviate from ideal behavior?

  Based on the graph below, choose the correct state3wvag1okm 2aen3zv3; .o 8 agqment that describes the relationship between pressure and temperature for a fixed mv kqz 3ea3a2ongw;m.o3g 8a1 vass and volume of a gas?

  The ideal gas equation is a formula 6 m 2yjey(j-vnthat combines the relationship between pressure, volume, temperature, and emnjjv-y2y 6(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 cma/:t9 scd0facf 5c,8iwcln2orrect calculation to determine the final volume of a fixec:scia ft/,cfd59wmlc0 2 8nad 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 wsoto ygkm 1 c e :l6ql2ahrk2( c3ht+3n:6yj9aith $N_2$, 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 g22 ti e7ffsgyoz-*.jr as $(N_2)$ 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 k91 llhh +dw1q9ib6x iolder cars. The airbag is deployed as lk91h9 +1lqwi b6 dihxa safety 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 behavior of an idealc 2is .s 9;o6rknkxa/k gas?. r/ s2 ;aokxkinkc9s6

  Under which conditions would a gas deviate the mo 0 cf:34(d1ovxs8olvgt ex v0bt1y lc)st from the ideal gas model?

  A sample of gas at a certain t 4r(jt9(ep -culih c1zemperature, 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 $T_2=\frac{1}{2}T_1$