For a fixed mass of gas at a constaniob 0+mpd/2 bjdh+4ynt temperature, what happens to the volume if the pressure of the gas i+ j/by+0 mipdoh24 dnbs doubled?

  Which of the following conditions maklaxmu)zz +t 8-es gases deviate from ideal behavior?

  Based on the graph be)(b fl j5,ujzqlow, choose the correct statement that describes the relationship between pressure and temperature for(zjq,5u b flj) a fixed mass and volume of a gas?

  The ideal gas equation is a formu .b gldh2 tl4jx0jls8*ovs2hz9ga83pla that combines the relationship between pressure, vogxhz4l3h jbav88 go 92d0 2s.s*tjpll lume, temperature, 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, what is the correct calcugbrcd+ e2zl.t ; u)0vslation to determine the final volume of a fixed mass of gasze2+td)su.0vg l;b rc:

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 w r5(yo4wa0 baiith $N_2$, 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 t9k16.div .ml1t a aqy$(N_2)$ 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 mtw2j fe /c/bi-j9 rb5cars. The airbag is deployed as a si /25mcjj-/ twberbf9afety 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 .,us2be g2 ii/fqf u)xof an ideal gas) u gbx iuis./2,2ffeq?

  Under which conditions would a gas deviate the most8phanc 19sd9y0r: :o: bh u.l2dnzhdv from the ideal gas model?

  A sample of gas at a certain temperature, pressure, and volw3rla*q;lz +;c ro4sf ume $(T_1,P_1,and V_1T)$ 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 $T_2=\frac{1}{2}T_1$