A 2.00 glass soda bottle filled only with air is tightly capped at 18degree C an

Question

A 2.00 glass soda bottle filled only with air is tightly capped at 18degree C and 718.0 mmHg. what is the pressure in the bottel? 82 mmHg b 849 mmHg 2830mmHg 607 mmHg 428 mmHg Which of the following statements are postulates of the kinetic-molecular theory of gases?Gas paniclcs are in constant, random motion the distance between gas particles is large in companion to the sue 3. The average kinetic energy of gas particles is proportional to the kelvin temperature 1 only 2 only 3 only 1 and 2 1.2. and 3 Sodium azide decomposes rapidly to produce nitrogen gas 2 NaN_3(t) rightarrow 2 Na(s) + N_2(g) What mass of sodium made will inflate a 60.01, airhag for a car to a prewire of 1.50 atm at 32degreeC? What is the pressure of a 49.4-L gas sample containing 1 04 mol of gas ai 36.4degreeC? The volume of a sample of gas measured at 65.01degreeC and 1.00 atm pressure is 2.00 L What must the final temperature be in order for the gas to have a final volume of 8 00 L at 1.00 atm pressure? 1079.0degreeC 260.0degree -13.0degreeC 16.3degreeC -188.5degreeC

Explanation / Answer

36.

We will use gas law for this problem. We will be calculating final pressure in this bottle. That is P2.

P1V1 = n1RT1(initial)    and P2V2 = n2RT2(final)

Since volume , mole and R are constant,

P1V1 = P2V2

P1V1/V2 = P2

18*718 / 71 = 182 mmHg.

37.

e. 1.2 and 3

38.

P = 1.50 atm

V = 60.0 L

T = 32 C = 305.15 K

R = 0.08206 L atm /molK

n = PV/RT = 1.50*60 / 0.08206*305.15 = 3.59 moles

These are the moles of sodium azide we require. Now we will convert it to grams.

Mass NaN3 = 3.59 moles* (65.00gNaN3/1 mol NaN3) = 234 g (65 is molar mass of Sodium azide)

39.

We will assume it as an ideal gas.

PV = nRT

V =49.4 L

n = 1.04 moles

R = 0.0821 L*atm/K*mol

T = 36.4C = 309.55 K

P = nRT/V

    = 1.04*0.0821*309.55/49.4 = 0.5350 atm = 4.06 * 10^2 mmHg

40.

T1 = 65C

V1 = 2.00 L

T2 = ?

V2 = 8.00 L

T1V1 = T2V2

65*2 = T2*8

T2 = 16.25C = 16.3°C

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