For a fixed mass of gas at a constant temperature, what h jdpsyxq 69f(yl;( :jbappens to the volume if the pressur9px(j l6yydsj : bf;q(e of the gas is doubled?

  Which of the following conditions makes gases deviate from ideal bet54avxb6:jskp7 o/eyhavior?

  Based on the graph below, chooz quq-d u+4m-avk en+4se the correct statement that describes the relationship between pressure and vd u4nm+qz-e-k+4 ua qtemperature for a fixed mass and volume of a gas?

  The ideal gas equation is a formula that ** )jem f25thtqgd juu .7k)ykcombines the relationship between pressure, volume, te kj)u2yt*5g7tmh .*)f jukedq mperature, 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, whsl .s,n:zp wl8lb q;u*at is the correct calculation to determine the final volume;pluq , bn:sslz w*.8l 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 inflate /ouiz+. g3 .niv;1bvhnxleh-d 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 xz(sghd3 p3*c$(N_2)$ 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 compoucq0m9::xi y pwnd found within the airbags of some older cars. The airiw0 :qcpy:x m9bag is deployed as a 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 witho5( z / ,kqp)kv kp5,pvmbias5 the behavior of an ideal gas5pok pmbvkaz,/5v, )qs ki(5p?

  Under which conditions would a gas deviate the most from the ideal gig:1d t/+2oeskvt;u qas model?

  A sample of gas at a certain tempekjyzvs3 dayl;)2f:.u+77 crcvh/u ea rature, 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 $T_2=\frac{1}{2}T_1$