A 6.00-m long rope is under a tension of 600 N. Waves travel along this rope at

Question

A 6.00-m long rope is under a tension of 600 N. Waves travel along this rope at 40.0 m/s. What is the mass of the rope? 1.00 kg 1.25 kg 2.25 kg 2.50 kg 1.12 kg One container is filled with Helium gas and another container is filled with Argon gas. If both containers are at the same temperature, which gas molecule's have the higher rms speed? (Argon has a higher atomic mass than helium.) the Helium gas the Argon gas they are both the same A sealed 26-m^3 tank is filled with 2000 moles of oxygen gas (O_2) at an initial temperature of 270 K. The gas is heated to a final temperature of 460 K. The ATOMIC mass of oxygen is 16.0 g/mol, and the ideal gas constant is R = 8.314 J/mol. K = 0.0821 L. atm/mol. K. The final pressure of the gas is closest to 0.29 MPa. 0231 MPa. 033 MPa. 0.34 Mpa. When a fixed amount of ideal gas goes through an adiabatic expansion Its internal (thermal) energy does not change. the gas does no work. no heat enters or leaves the gas. its temperature cannot change. A 648-g empty iron kettle is put on a stove. How much heat, in joules, must it absorb to raise its temperature from 15.0 degree C to 37.0 degree C? (The specific treat for iron is 113 cal/kg. C degree, 1 cal = 4.190 J) 6740J 11.300J 1610J 16,100 J If 3.0 g of water at 20.00 degree C is to be vaporized, how much heat must be added to it? The specific heat of water is 1.0 cal/g.K, its heat of fusion is 80 cal/g. and its heat of vaporization is 539 cal/g. 1100 cal 1100 kcal 1300 cal 1900 cal

Explanation / Answer

5.solution

Velocity = sqrt (tension / mass per length)

V2 = T*L / m

m = T*L / V2

m = 600*6m / 402

m =2.25kg

6.solution

At the same temperature, the average value of the translational kinetic energy [(1/2) mv2] will be the same for both helium and argon. Argon has a larger mass so it will have a smaller value of v2 or vrms. Helium has a smaller mass so it will have a larger value of <v2> or vrms.

7.solution

Since we're told the oxygen is behaving as an ideal gas, use the ideal gas law:

PV = nRT

Solve for P: P = nRT/V

n = 2000 moles

R = 8.314 m3·Pa·K-1·mol-1
(use the value of R with units Pa and m3)

T= 460 K
(use the final T for initial V)

V = 26 m3

I got P = 294187.69 Pa = 0.29 MPa

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