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Anni [7]
3 years ago
10

A mass of 0.1 kg of helium fills a 0.2 m3 rigid tank at 350 kPa. The vessel is heated until the pressure is 700 kPa. Calculate t

he a) the temperature change of helium [deg. C], and b) the total amount of heat required for this process [kJ].
Physics
1 answer:
QveST [7]3 years ago
3 0

Explanation:

(a)   First, we will calculate the number of moles as follows.

       No. of moles = \frac{\text{mass}}{\text{molar mass}}

Molar mass of helium is 4 g/mol and mass is given as 0.1 kg or 100 g (as 1 kg = 1000 g).

Putting the given values into the above formula as follows.

       No. of moles = \frac{\text{mass}}{\text{molar mass}}

                             = \frac{\text{100 g}}{4 g/mol}  

                             = 25 mol

According to the ideal gas equation,

                           PV = nRT

or,       (P_{2} - P_{1})V = nR (T_{2} - T_{1})

          (6.90 atm - 3.45 atm) \times 200 L = 25 \times 0.0821 L atm/mol K \Delta T

          \Delta T = 336.17 K

Hence, temperature change will be 336.17 K.

(b)   The total amount of heat required for this process will be calculated as follows.

                   q = mC \Delta T

                      = 100 g \times 5.193 J/g K \times 336.17 K

                      = 174573.081 J/K

or,                  = 174.57 kJ/K        (as 1 kJ = 1000 J)

Therefore, the amount of total heat required is 174.57 kJ/K.

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+1.11\mu C

Explanation:

A charge located at a point will experience a zero electrostatic force if the resultant electric field on it due to any other charge(s) is zero.

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where r_2 is the distance of Q_2 from the origin, r_3 is the distance of Q_3 from the origin and k is the electrostatic constant.

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\frac{Q_2}{0.025^2}=\frac{2.18*10^{-6}}{0.035^2}\\\\hence;\\\\Q_2=\frac{0.025^2*2.18*10^{-6}}{0.035^2}\\

Q_2=\frac{0.00136*10^{-6}}{0.00123}=1.11*10^{-6}C\\\\Q_3=+1.11\mu C

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