For a fixed mass of gas at a constant temperature, what happensdt7qjb p( i 7ep6.9azfv/us5 k to the volume if the pressure of the gas ispj edqu5a/ zbk vfip(7976 .st doubled?

  Which of the following conditions mahowe(z0ym p4 l,+x rn5gi)1 bqkes gases deviate from ideal behavior?

  Based on the graph below, choose the correct statement that descre y pjw ,damww+,4b1n+ibes the relationship between pressure and temperature for a f,1+a+ b,y4djw npmw ewixed mass and volume of a gas?

  The ideal gas equation is a formula that/rmgvn4+zcnl+ :: ntog 3v5fm combines the relationship between pressure, volume, temperature, and t+rn3n fvcn/gz vtm+::5omgl4 he 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 to deterf;w5mn+ i5 ndimine the final vold5ni5;f +wmi nume 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 3 h641m 9debq yx01ldn8w h+n,ruroz7bm-fsu inflated 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 5 imxwsz*xt *1 xk9a ,*bmu+gg$(N_2)$ 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 7u -67dpmfwru airbags of some older cars. The airbag is deployed as a safety feat6r f7u-mu7dpwure 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 ga9,x26 slcpn. ek8 jitsses most closely aligns with the behavior of an ideal gas?,2.j n ktsicsx9e86pl

  Under which conditions would a gas deviate theb5r uz 95 nej7rgm-m9b most from the ideal gas model?

  A sample of gas at a certain temperature, pressure, andzqc0-l2liv c ;b:zhd / 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 $T_2=\frac{1}{2}T_1$