Question

1. How many moles of gas must be forced into a 4.8 L tire to give it a gauge pressure of 32.4 psi at 30 ∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.5 psi so that the total pressure in the tire is 46.9 psi . Express your answer using two significant figures. n = _____ mol

*** different kind of question***

2. What volume of O2 at 988 mmHg and 21 ∘C is required to synthesize 19.0 mol of NO?

Express your answer to three significant figures and include the appropriate units. volume of O2 =

***LAST question please answer***

3. High-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 Pa) to about 60,000 kPa (60,000,000 Pa). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 2.40×10⁸ Pa , what is its running pressure in torr?

Express the pressure numerically in torr. 2.40×10⁸ Pa = ________ torr

Answer 1

Given total pressure = 46.9 psi = 3.19 atm

Now, We can use PV = nRT

V = 4.8 L

R = 0.082 L atm/ mol K

T = 30 + 273 = 303 K

So, 3.19 x 4.8 = n x 0.082 x 303

n = 0.616 moles

(2)

The reaction is N2+02 ---> 2 NO

Moles of O2 = 1/2 x moles of NO = 19/2 = 9.5 moles

Volume = nRT/P = (9.5 x 0.082 x 294 K ) / (988/760)

= 176 L

(3)

760 torr = 101,325 Pa

Multiply the factor by the given pressure.

2.40 x 10^8 Pa x 760 torr / 101,325 Pa = 1.80 x 10^6 torr

according to cheg rules only one question should be answered .thats why i answered 1 st one. Now i answered 3 questions for u ,pls give good rating