This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
ScanSolve AI Answer
Fresh day ThegirlGodishelping🥰💙🫠, let's solve. Step 1: Convert the temperature from Celsius to Kelvin. The given temperature is 100^. T = 100^ + 273.15 = 373.15 K Step 2: Calculate the number of moles of Oxygen gas (O_2). The mass of Oxygen gas is 16.0 g. The molar mass of Oxygen gas (O_2) is 2 × 16.00 g/mol = 32.00 g/mol. n = massmolar mass = 16.0 g32.00 g/mol = 0.50 mol Step 3: Apply the formula for work done during isothermal compression. For an isothermal process, the work done on the gas is given by: W = nRT ((V_i)/(V_f)) Where: n is the number of moles R is the ideal gas constant (8.314 J/(mol·K)) T is the temperature in Kelvin V_i is the initial volume V_f is the final volume The problem states that the volume is halved, so V_f = (1)/(2)V_i. Therefore, (V_i)/(V_f) = (V_i)/(1)2V_i = 2. Step 4: Substitute the values and calculate the work done. W = (0.50 mol) × (8.314 J/(mol·K)) × (373.15 K) × (2) W = 0.50 × 8.314 × 373.15 × 0.693147 W ≈ 1074.00 J Rounding to the nearest whole number, the work done is 1074 J. The final answer is 1074 J. What's next?