A car tyre is filled with nitrogen gas at 35 psi at 27°C. It will burst if pressure exceeds 40 psi. The temperature in °C at which the car tyre will burst is--------------. (Rounded – off to the nearest integer)

2 Views | Posted a month ago

Asked by Shiksha User

1 Answer

Answered by

Vishal Baghel | Contributor-Level 10

a month ago

$\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}} \Rightarrow \frac{35}{300} = \frac{40}{T_{2}}$

$∴ T_{2} = \frac{40 \times 300}{35} = 342.85 K$

$T_{2} (° C) = 69.707 \approx 70 ° C$

0 Upvotes 0 Downvotes

Similar Questions for you

Correct order of van der Waals constant b of given gases is

alok kumar singh

Correct order of van there Waals constant b for gases is CO₂ > N₂ > O₂ > H₂ > He

Match the following.

	Column I (Ores)		Column II (Formula)
(A)	Fluorspar	(p)	Al₂O₃.2H₂O
(B)	Cryolite	(q)	CaF₂
(C)	Bauxite	(r)	MgCO₃.CaCO₃
(D)	Dolomite	(s)	Na₃[AIF₆]

alok kumar singh

(A) Fluorspar – CaF₂

(B) Cryolite – Na₃ [AlF₆]

(D) Dolomite – MgCO₃.CaCO₃

A gas at 300 K and 10 bar has molar volume 10% more than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor (Z) is

alok kumar singh

Kindly go through the solution

Since V_Real> V_ideal

So, Z = V_Real > 1. V_ideal

For an ideal system at thermal equilibrium, the velocity distribution of the constituting particles

alok kumar singh

The Answer is Maxwell? Boltzmann distribution

Which of the following gases can be liquefied most easily?

alok kumar singh

NH₃ can be liquefied most easily due to presence of strong intermolecular H-bonding among NH3 molecules.