If 84.5 mol of an ideal gas occupies 21.5 L at 305 K, what is the pressure of the gas? pressure: atm

98.367 atm

Explanation:

For this, you must use the equation PV=nRT. Since you are looking for P, rearrange the equation so that P= nRT/V.

Now collect the information you have:

n (mol) = 84.5

R (ideal gas constant to find atm not every case) = .08206

T (temperature) = 305 K (always convert to kelvin)

V (volume in liters) = 21.5

Now Use P= (85.5 mol)×(.08206)×(305 K)/(21.5) to get your answer in atm

-8024.832 J

Explanation:

The amount of heat energy lost or released, Q, can be calculated thus;

Q = m × c × ∆T

Where;

Q = amount of heat lost (J)

m = mass of substance (g)

c = specific heat capacity (J/g°C)

∆T = change in temperature (°C)

According to this question,

Q = ?

m = 24.3 g

c of Gold = 0.129 J/g°C

∆T = 20°C - 2580.0°C = -2560°C

Using Q = m × c × ∆T

Q = 24.3 × 0.129 × -2560°C

Q = -8024.832 J

This means that 8024.832 J of energy is lost or released.