The temperature of 2.97 mol of a monatomic ideal gas is 511 K. The internal energy of this gas is doubled by the addition of heat. How much heat is needed when it is added at (a) constant volume and (b) constant pressure

The heat needed when volume is constant is 18926.9 J

The heat needed when pressure is constant is  31544.8 J

Explanation:

Step 1: Data given

Number of moles of a monoatomic gas = 2.97 mol

Temperature of the gas = 511 K

The internal energy of this gas is doubled by the addition of heat.

Step 2:

At a constant volume workdone is 0.

Q = ΔU + W

Q = 3/2 n*R*T

⇒n = the number of moles = 2.97 moles

⇒R = the gas constant = 8.314 J/mol*K

⇒with T = the temperature = 511 K

Q =  3/2 *2.97 * 8.314 * 511

Q = 18926.9 J

Step 3: At a constant pressure workdone is:

W = p*V

W = n*R*T

 ⇒ Q = ΔU + W

Q = 3/2 *nRT + nRT

Q = 18926.9 + 2.97 * 8.314 * 511

Q =  31544.8 J

The heat needed when volume is constant is 18926.9 J

The heat needed when pressure is constant is  31544.8 J

no, i was listening to water by schoolboy q while and i saw this question

explenation:

water isn't wet. wetness is a description of our experience of water; what happens to us when we come into contact with water in such a way that it impinges on our state of being. we, or our possessions, 'get wet'. a less impinging sense experience of water is that it is cold or warm, while visual experience tells us that it is green or blue or muddy or fast-flowing. we learn by experience that a sensation of wetness is associated with water: 'there must be a leak/i must have sat in something.'

the answer would be a