For a fixed mass of gas at a constant temperature, what happens to the vo5f tjs5bs.my1ff 3fn :lume if tn5fyt5f 3j:fbs.1f s mhe pressure of the gas is doubled?

  Which of the following conditions makr9 3pe bev qf9-tsjk/ eun4*fp2 )kmj1es gases deviate from ideal behavior?

  Based on the graph below, choose the correct statement that describes thx92gd imk t)i(e relationship between pressure and temperature for a fixed mass and volume of ag9(dkt2x )iim gas?

  The ideal gas equation is a formula that combines the relationship between dup 2u*tz.6z)utm b-ipressure, volume, temperature, and the number of moletu)t ibz-6 z.upum2d *s.
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 determine3 zkob9btq34 f the final volume of a fixed mk9f 4b3t zqbo3ass 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 wddh6q9 jnj3 j9e(u f.qy+)8qkvj bpu:ith $N_2$, 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 4-fynt vtwf,d3.rsp 3 $(N_2)$ 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 compo d4w2 mfk-sdf 3s7etr)und found within the airbags of some older cars. The airbag is deployed as a safety feature in the event of an accident. In this application, the sodium azide decomposes rapidly, and the gas fordwr 4)2 k fd73-tsfesmmed 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 gaid09a r8pi2oqses most closely aligns with the behavior of an ideal ga9 rqp8 iida02os?

  Under which conditions would a gas denr pc2k9t55d bviate the most from the ideal gas model?

  A sample of gas at a certain temperatugvf8d 80rizfb* j; /etre, 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 $T_2=\frac{1}{2}T_1$