For a fixed mass of gas at a constant temperaturehik2-md *46 udgz 2jd3py hd:i, what happens to the volume if the pressure of theyduzd3m hi k:pgd4j-22* 6 hid gas is doubled?

  Which of the following cai) 7 y:6yyjvi v0zi*bonditions makes gases deviate from ideal behavior?

  Based on the graph below, choose the correct statement that describes ztna ek;- u3v8the relationship betw uv;3aen-8 ztkeen pressure and temperature for a fixed mass and volume of a gas?

  The ideal gas equationykwn* 2*j8 7y x;gu,oddb m(gd is a formula that combines the relationship between pressure, volume, temperature, and the number of mowodm,j*d 8dn(k ;uy b2gxy7*g les.
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 calcueeri2ed6n. 7 elation to determine the final volume of a fixen.rie e267eded 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 wit3a+st5yij:.1ot6idl viw 4 l jh $N_2$, 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 gd9*3 wgeh :wi wnjh,c j.)ss,a8p8on fas $(N_2)$ 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 comp ;dsf(-zxbwvj 6x7 0oround found within the airbags of some older cars. The airbag is deployed as a safety feature in theof(zvw; b0x sr7x-j6d 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 closelct5fzaqq4z f4+/ a8lx y aligns with the behavior of an ideal gasf/cq4t5l4f ax+z8q za ?

  Under which conditions would a gas deviate the mospu4+b fsd+lci/s +rkvn; 8(k vo*u x+mt from the ideal gas model?

  A sample of gas at a certain temperak)hu)zgn: ,-ul-u lykou ,/heture, 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 $T_2=\frac{1}{2}T_1$