Question

1. On a summer day, you take a road trip through Death Valley, California, in an antique car. You start out at a temperature of 21°C, but the temperature in Death Valley will reach a peak of 51°C. The tires on your car hold 15.6 L of nitrogen gas at a starting pressure of 249 kPa. The tires will burst when the internal pressure (Pb) reaches 269 kPa. Answer the following questions and show your work.

Answer 1

• How many moles of nitrogen gas are in each tire?
• What will the tire pressure be at peak temperature in Death Valley?
• Will the tires burst in Death Valley? Explain.
• If you must let nitrogen

Answer 2

"How many moles of nitrogen gas are in each tire?"

use the ideal gas law PV=nRT

"What will the tire pressure be at peak temperature in Death Valley?"

use P1V1/T1=P2V2/T2

Answer 3

lol you totally copied that from another question like mine :p
I see what you did there xD

Answer 4

THE QUESTION IS TRICKY SO I search it

Answer 5

i think for the second one ichlie is right...

Answer 6

what about the first one though?

Answer 7

P = pressure (249 kPa = 2.4574 atm)

V = 15.6 L

n = moles

T = Temp in Kelvin (21 deg C = 273.15 + 21 = 294.15 Kelvin)

R = gas constant = 0.0821 L atm mol^-1 K^-1

i hope no one has this on other answers

Answer 8

@Somy
and http://howtochangeatireonyourcar.blogspot.com/2010/11/please-help-with-chemistry-problem-so.html
xD

Answer 9

:/

Answer 10

well there are ways to find moles ..u can use number of moles = mass/molar mass
but there's no mass given :(......u can also find it by using the formula V = moles * 24dm^3 but it can't be used on this one...so i m also confused....:l

Answer 11

n = 1.5874 moles N2

n = 1.59 mol

Answer 12

the answers are on the website you gave me

Answer 13

what exactly do u not get here?

Answer 14

nvm lol you were all correct I got it -.-'

Answer 15

On a summer day, you take a road trip through Death Valley, California, in an antique car. You start out at a temperature of 21°C, but the temperature in Death Valley will reach a peak of 51°C. The tires on your car hold 15.6 L of nitrogen gas at a starting pressure of 249 kPa. The tires will burst when the internal pressure (Pb) reaches 269 kPa. Answer the following questions and show your work.

lets see whats known
T1= 21°C
T2= 51°C
V1= 15.6 L
P1= 249 kPa
Bursting pressure= 269 kPa

so these are known to you
now qs
How many moles of nitrogen gas are in each tire?
- We know that it can hold 15.6 L
so we are going to use
PV=nRT
here, unknown is 'n' so lets make it as a subject of this formula
n= PV/RT
P1, V1, R (according to units of the rest of the members of formula) and T1 are known to you
so put them into formula and find mole of nitrogen
**********************************************


What will the tire pressure be at peak temperature in Death Valley?
\[\frac{ P_1 }{ T_1 } = \frac{ P_2 }{ T_2 }\]
you have P1, T1 and T2 given to you
do find P2 using this formula
**********************************************


Will the tires burst in Death Valley? Explain.
The Pressure at which tire will burst is given to you
compare it with P2 that you will find in 2nd section
and see, if its less than bursting pressure- it will not burst, if its equal or more than that- it will burst
*************************************************

Finish till here, then will move to this last one
If you must let nitrogen gas out of the tire before you go, to what pressure must you reduce the tires before you start your trip? (Assume no significant change in tire volume.)

Answer 16

owh lol didnt see ur response :3

Answer 17

lol is ok thank you though ^.^

Answer 18

no problem :)

Answer 19

(can you guys share medals because you know I cant give more than 1 medal :))

Answer 20

sure :D

Answer 21

thanks

Answer 22

Thanks..