For a fixed mass of gas at a constant tempeawevx) cg-7e 8r8 4fcjrature, what happens to the volume if the pressure of the gas r7g e)x4j 8cc-v e8fwais doubled?

  Which of the following conditions makes gases deviate from ideay5b05y;s jzxa l behavior?

  Based on the graph below, choose the correct statement that p7m t9:l1r encdescribes the relationship between pressure and temperature for a fixed mass and volumplc:r men t971e of a gas?

  The ideal gas equation is a formula that combines the qhf u5lox*a1uey13 0b0xnc hax3 bt,/relationship between pressure, voluhna ecxfa hxu*5/ux lt,b1oy 3b0q130me, 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 iwg0d+awoh c lm3 w)6w1s the correct calculation to determine the final volume 1w0+ m)6dlcwhgwaw3o 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 inflated wix9+dlmk ;j0f vyrgqar; / 01tmth $N_2$, 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 gai3z fjlcf) .u;s $(N_2)$ 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 compow0ztwr wu93u +.ooo* ound found within the airbags of some older cars. The airbag is deployed as a safety feature in the u+ r0z9*oowwt wu3oo. 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 gaseaq t5b. ss4ha.s most closely aligns with the behavior of an ideal gas4 bta.5qas.s h?

  Under which conditions would a gas deviate the most from the ideal gasr/ khjcmcf 3(+s p,1fa model?

  A sample of gas at a certain temperature, pressujaex/x x14hutr1t ,0.fl,s 0 xfy: zqire, 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 $T_2=\frac{1}{2}T_1$