For a fixed mass of gas at a constantwjnvb4.2 msx1 temperature, what happens to the volume if the pressurwb 2jsmx4 v1n.e of the gas is doubled?

  Which of the following conditions makes gases de rz l)*a uavn vhpd(s.8)*loy+viate from ideal behavior?

  Based on the graph below, xnz0sz;) b,h86zeqz2btu8+4oyg mk v choose the correct statement that describes the relationship between pressure and temperature for a fe08 gqzu4+s 26k,zbzhx8v; ymnzbt)oixed mass and volume of a gas?

  The ideal gas equation is a formula that combines the relationshib23.kfh1lql o p between pressure, volume, temperature, and 2kbfo3.q hll1 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 tnln t:+l5/)h )dhxpg*qpb vj ,o determine the final volume of a fixed mass of gas: *l:xptnhnj ,/5h)dgp)+q lvb

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 infl6k tx 8,dgu8cuated 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 g+g u8ab79qsvd ssbdl pe10/:9i qip)aas $(N_2)$ 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 ai;7tca ky j-i5srbags of some older cars. The airbag is deployed as a safety feature in the event of an accident. In this application, the s kjcs5i7y- ta;odium 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 aqn s9s:0x y f3ch)+fkclosely aligns with the behavior of an ideal ga9+ 3s:f0snyxc ) hkfqas?

  Under which conditions would a gas deviate the most from the hgd qdg0l)m8rxmyvzlk67 1wb60 d;g .ideal gas model?

  A sample of gas at a certain tem.tzq)mh1 q6f 4*whtni perature, 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 $T_2=\frac{1}{2}T_1$