For a fixed mass of gas at a constant temperature, what happens qc 5* qqabi4z:to the volume if the pressure of 4:bq*5 iazqcq the gas is doubled?

  Which of the following conditions makes s1k r/h:j whi,h4 gcjp z+ r)zs0dqs,;gases deviate from ideal behavior?

  Based on the graph below, choose the correct statement that describ i 6vtfqrxxsb-h :3le g0-; cnpjx8w(6es the relationt v:w38- 6bx6-fnl;c(pjixq0 rsg ehxship between pressure and temperature for a fixed mass and volume of a gas?

  The ideal gas equation is a form+ /bzvkm:c, b;s:tafs pev u6)z1e e0bula that combines the relationship between pressure, volume, temperature, and the numbe:bpefe zv:bsck bm0 a,z u+)t vs1/e;6r 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 corb+wl5kae,8 ea rect calculation to determine the final volume of a fixa 8k +eea5blw,ed 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 w2 mwa)e 0e2y(o:slybb 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 gaw)mqd y2j7j -ys $(N_2)$ 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 co 1v/ ,on)hipk63i oxvcmpound found within the airbags of some older cars. The airbag is d31kn)xv ,6 /iohivc opeployed as a safety 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 c.z hy,h00r xbmost closely aligns with the behavior of an ideal gas?rhc.y, h0b x0z

  Under which conditions would a gas deviate the most froa fbc7xgf)7i1m the ideal gas model?

  A sample of gas at a certain temperature, pressur6b 1d:+0 b duy8my j.cylhxb-oe, 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 $T_2=\frac{1}{2}T_1$