This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey Ni_Fe_Mi✨, good to see you again. Here are the solutions to your practice questions: 1. Calculate the molar mass of the gas. Step 1: Determine the number of moles at STP. At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 L. Given volume V = 0.280 L. n = (V)/(Molar volume at STP) = 0.280 L22.4 L/mol n = 0.0125 mol Step 2: Calculate the molar mass. Molar mass (M) is the mass (m) divided by the number of moles (n). Given mass m = 0.400 g. M = (m)/(n) = 0.400 g0.0125 mol M = 32.0 g/mol The molar mass of the gas is 32.0 g/mol. 2. What is the new volume? Step 1: Convert initial temperature to Kelvin. Given initial temperature T_1 = 25 \,^. T_1 = 25 + 273.15 = 298.15 K Step 2: Calculate the final temperature in Kelvin. The temperature increases by 5 \,^. T_2 = (25 + 5) \,^ = 30 \,^ T_2 = 30 + 273.15 = 303.15 K Step 3: Apply Charles's Law. Since pressure is constant, we use Charles's Law: (V_1)/(T_1) = (V_2)/(T_2). Given initial volume V_1 = 0.62 L. V_2 = V_1 ((T_2)/(T_1)) = 0.62 L (303.15 K298.15 K) V_2 = 0.62 L × 1.01677 V_2 ≈ 0.63 L The new volume is 0.63 L. 3. Calculate the approximate molar mass of a gas. Step 1: Convert temperature to Kelvin. Given temperature T = 30 \,^. T = 30 + 273.15 = 303.15 K Step 2: Convert pressure to atmospheres. Given pressure P = 780 torr. P = 780 torr × 1 atm760 torr ≈ 1.0263 atm Step 3: Calculate the molar mass using the ideal gas law in terms of density. The ideal gas law can be written as PM = RT, where M is molar mass, is density, and R is the ideal gas constant (0.08206 L·atm/(mol·K)). Given density = 3.33 g/L. M = ( RT)/(P) M = (3.33 g/L)(0.08206 L·atm/(mol·K))(303.15 K)1.0263 atm M = 82.91 g·atm/mol1.0263 atm M ≈ 80.8 g/mol The approximate molar mass of the gas is 80.8 g/mol. Drop the next question! 📸