Albedo is reflected power over incident power, here reflected is 40, incident is 100, hence 0.4.
CloseFor this, we need to use the equation \(L = \frac{Q}{m}\), so we have \(Q = 0.25 \cdot 3 \cdot 10^5\), which results in A.
CloseAverage kinetic energy is related to the temperature, hence we can say that the temperature has been increased.
CloseWe need to make sure that our temperatures are in Kelvin, as that's the only time we can use the ideal gas equations. So our temperature (thus the pressure) increases by a factor of \(\frac{(273 + 100)}{(273 + 50)} = \frac{373}{323}\), which is obviously not 1, 1.5, or 2, hence \(B\) must be correct.
CloseUsing Boyle's Law:
\[ P_1 V_1 = P_2 V_2 \]
where:
Rearranging for \( P_2 \):
\[ P_2 = \frac{P_1 V_1}{V_2} = \frac{(2.00)(4.00)}{2.00} = 4.00 \, \text{atm} \]
CloseUsing Charles's Law:
\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]
where:
Rearranging for \( V_2 \):
\[ V_2 = V_1 \frac{T_2}{T_1} = 3.00 \cdot \frac{450}{300} = 4.50 \, \text{L} \]
CloseThe Ideal Gas Law is:
\[ PV = nRT \]
where:
Rearranging for \( V \):
\[ V = \frac{nRT}{P} \]
Substitute the values:
\[ V = \frac{(0.50)(8.31)(300)}{202650} \approx 6.15 \, \text{mL} \]
CloseThe Ideal Gas Law is:
\[ PV = nRT \]
where:
Rearranging for \( n \):
\[ n = \frac{PV}{RT} \]
Substitute the values:
\[ n = \frac{(101325)(2.00 \times 10^{-3})}{(8.31)(273)} \approx 0.089 \, \text{mol} \]
The molar mass \( M \) is:
\[ M = \frac{\text{mass}}{n} = \frac{2.00}{0.089} \approx 22.5 \, \text{g/mol} \]
CloseThe total internal energy of a monatomic ideal gas is given by:
\[ U = \frac{3}{2} nRT \]
where:
Substitute the values:
\[ U = \frac{3}{2} (1.00)(8.31)(300) = \frac{3}{2} \cdot 2493 \approx 3740 \, \text{J} \]
CloseUsing the Ideal Gas Law:
\[ PV = nRT \]
Rearranging for \( n \):
\[ n = \frac{PV}{RT} \]
where:
Substitute the values:
\[ n = \frac{(2.50)(10.0)}{(0.0821)(298)} \approx \frac{25.0}{24.5} \approx 1.02 \, \text{mol} \]
The mass of the gas is:
\[ \text{mass} = n \cdot \text{Molar Mass} = (1.02)(28.0) \approx 28.5 \, \text{g} \]
CloseReal gases deviate from the ideal gas model because their particles have a finite size (leading to excluded volume effects) and because intermolecular forces (such as Van der Waals forces) affect particle interactions.
CloseAt very high pressures, the finite volume of gas molecules becomes significant, and the pressure exerted by the gas is higher than what is predicted by the ideal gas law. This deviation is a result of the "excluded volume" effect described in the Van der Waals equation.
Close