For a fixed mass of gas at a constant tempey9fxyvc17,+qw9g3 jj ds)ubsrature, what happens to the volume if the pressure )9vb wqjjsfsy,1 y9 gud3x7c+of the gas is doubled?

  Which of the following conditions makes gases deviate from ideal beha/a kqhmoaf 9v,q-0 z7x)p2pr rvior?

  Based on the graph below, choose the correct statement that des +hqb,1uqd- cccribes the relationship between pressure and temperature focqh1d ,cu-q+br a fixed mass and volume of a gas?

  The ideal gas equation is a formula that combines the r5d u8fq+ryngdg6j;3x * dgl+selationship between pressure, volume, temperature, and the number of r *gxdn56+jqdd+g8gsu3l ;yf 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 calculati l/j)1ykdeh 9pon to determine the final volume of a fixed mass of gas:he9l jd/pky1)

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 with:u4 s e9mn*l+x h+evfi $N_2$, 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 g kr 801jxl acg8o(+olvmd .v7f bfp6fz:2-aoz as $(N_2)$ 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 somyet/g .:g7l) e6zptoae older cars. The airbag is deployed as a safety featuroylg:te6e7.) tzga / pe 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 clf;0ifp wt x*ld;2d0cv*.v-iks .ug9 avb5k wjosely aligns with the behavior of an ideal gas?ixs wb*.;a2vvk0tj lwvdg .5 09c ik*u-pf d;f

  Under which conditions would a gas deviate the most from the ideal gas muk;bee bcwr.8 +1ail4b4w2 jvodel?

  A sample of gas at a certain temperature, pressure, an:wb31ei dpbfw.lz32t d 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 $T_2=\frac{1}{2}T_1$