Nov-29-2019 03:37 AM
Dec-10-2019 11:01 AM
Dec-10-2019 10:55 AM
jspringator wrote:
..........What we don’t know is whether the weight chart extends to pressures less than 65psi.
Dec-10-2019 05:15 AM
Dec-10-2019 05:01 AM
4x4van wrote:
Your math makes sense, and I understand your reasoning. I just wanted to point out that I have heard that you shouldn't go lower than the lowest pressure on the chart, regardless of weight carried. True? I have no idea, just relating what I've heard.;)
Dec-09-2019 08:29 AM
Dec-09-2019 08:23 AM
jspringator wrote:Your math makes sense, and I understand your reasoning. I just wanted to point out that I have heard that you shouldn't go lower than the lowest pressure on the chart, regardless of weight carried. True? I have no idea, just relating what I've heard.;)
The tires are rated for 2,755 lbs per tire at 65 psi. Actual loaded weight is 2,320, or 870 pounds under max weight for both tires on the front. The rear is rated for 2755 X 2= 5,510 per dual or 11,020 for both rear sides. The actual loaded weight for the rear is 8,240. That is why it performs better with lower pressures.
The chart didn't go below 65 psi, so I extrapolated the weight difference per tire in 10 psi increments in the other direction. The weight increase between 65 to 75 is 285 pounds. The difference between 75 and 85 is an increase of 275 pounds. The difference between 85 and 95 is 325 pounds. Based on the foregoing, I would believe the reduction in weight carrying per tire would be less than 300 pounds per tire for a 10 psi decrease in pressure, or 55 psi. Even that would give me a 200 pound margin of safety on the front, and 1,580 in the rear. So I settled on what I believe to be 60 psi, that will leave an even greater margin of safety.
Dec-05-2019 05:20 PM
Dec-05-2019 01:27 PM
jspringator wrote:Winnebago's recommendation (I'm assuming on the Federal tag on/near the driver's door) is NOT for the entire Sightseer line, but rather for your specific model, based on it's maximum GVWR, which is 14,800. If your rig actually weighs less than that max, then it would make sense that it handles better at slightly lower pressures.
I noticed on my last trip the MH handeled very well when the TPMS showed the hot pressure at 66-69 across the range of 6 tires. My pump was showing the pressure at 60psi when cold inflated, but the TPMS showed 55. Winnebago recomends 65, but the loading charts for the tires show a huge margin of safety at actual weights at the scale. I thnk the issue with mine is that it is a shorty at 27', and I surmise the pressure of 65 is for the entire Sightseer line. My gage, the tire pump and my TPMS all give different readings.
Actually the improvement in handling at these pressures was nothing short of remarkble. I felt noticably less fatigued. I don't remember the tire temperature, but the alarm didn't go off. I'll check that next trip.
Dec-04-2019 04:24 AM
Nov-30-2019 07:10 AM
Nov-30-2019 05:57 AM
Nov-30-2019 05:17 AM
Octaneforce wrote:2bzy2c wrote:Captain_Happy wrote:
Something else to consider is inflating your tire with Nitrogen instead of pain air. Nitrogen doesn't heat up like plain air does. You stated that you F53 handles pretty good with PSI at 80 PSI when you start out, but as your tires heat up the handling changes. I've owned 2 F53 and they both handled badly.
Bzzzzzt WRONG!
There is virtually no difference between N2, O2, Air and Co2 thermal expansion rates.
"I'll take Thermal Expansion for $100 Alex."
Geek speak on the subject -->
Ideal Gas Law: PV = nRT
This formula is the "Ideal Gas Law Formula." Although there is no such thing as an ideal gas the formula is pretty accurate for N2, CO2, and oxygen as we assume that the gas molecules are point masses and the collisions of the molecules are totally elastic. (A completely elastic collision means that the energy of the molecules before a collision equals the energy of the molecules after a collision, or, to put it another way, there is no attraction among the molecules.) The formula becomes less accurate as the gas becomes very compressed and as the temperature decreases but here "very compressed" pressures are well above even the highest tire pressures and "decreased temperatures" are extremely cold, too cold for tires. There are some correction factors for both of these factors for each gas to convert it to a Real Gas Law Formula, but the Ideal Gas Law is a good estimation of the way N2, CO2 and "air" should react through temperature changes. What does all this mean? It simply means that "air", nitrogen vapor, and CO2 vapor should all react pretty much the same within normal tire pressures (0-120 PSI) and temperatures.
In the hvac business we use nitrogen for leak down tests under the assumption that it doesn't fluctuate in pressure like compressed air will. However we use pressure way beyond that of a tire (500-600psi). I guess this is within the theory you provided.
Why do race car drivers bother to use nitrogen in their tires? Is it a myth?
Nov-30-2019 04:34 AM
Octaneforce wrote:2bzy2c wrote:Captain_Happy wrote:
Something else to consider is inflating your tire with Nitrogen instead of pain air. Nitrogen doesn't heat up like plain air does. You stated that you F53 handles pretty good with PSI at 80 PSI when you start out, but as your tires heat up the handling changes. I've owned 2 F53 and they both handled badly.
Bzzzzzt WRONG!
There is virtually no difference between N2, O2, Air and Co2 thermal expansion rates.
"I'll take Thermal Expansion for $100 Alex."
Geek speak on the subject -->
Ideal Gas Law: PV = nRT
This formula is the "Ideal Gas Law Formula." Although there is no such thing as an ideal gas the formula is pretty accurate for N2, CO2, and oxygen as we assume that the gas molecules are point masses and the collisions of the molecules are totally elastic. (A completely elastic collision means that the energy of the molecules before a collision equals the energy of the molecules after a collision, or, to put it another way, there is no attraction among the molecules.) The formula becomes less accurate as the gas becomes very compressed and as the temperature decreases but here "very compressed" pressures are well above even the highest tire pressures and "decreased temperatures" are extremely cold, too cold for tires. There are some correction factors for both of these factors for each gas to convert it to a Real Gas Law Formula, but the Ideal Gas Law is a good estimation of the way N2, CO2 and "air" should react through temperature changes. What does all this mean? It simply means that "air", nitrogen vapor, and CO2 vapor should all react pretty much the same within normal tire pressures (0-120 PSI) and temperatures.
In the hvac business we use nitrogen for leak down tests under the assumption that it doesn't fluctuate in pressure like compressed air will. However we use pressure way beyond that of a tire (500-600psi). I guess this is within the theory you provided.
Why do race car drivers bother to use nitrogen in their tires? Is it a myth?
Nov-30-2019 02:47 AM