can u help me w this question The common laboratory solvent diethyl ether (ether) is often used to purify substances dissolved in it. The vapor pressure ofdiethyl ether, CH3 CH₂ OCH₂ CH3, is 463.57 mm Hg at 25 °C.In a laboratory experiment, students synthesized a new compound and found that when 16.23 grams of the compound weredissolved in 176.4 grams of diethyl ether, the vapor pressure of the solution was 452.86 mm Hg. The compound was also found tobe nonvolatile and a non-electrolyte.What is the molecular weight of this compound?(Diethyl ether = CH3 CH₂ OCH₂ CH3 = 74.12 g/mol)Molecular weight =g/mol

In the first step, we identify the solute is non volatile and the solvent is diethyl ether.next we calculate moles of solvent by dividing mass by molar mass.The vapor pressure of pure diethyl ether at a certain temperature is 463.57 mmHgThe amount of solute and diethyl ether in a solution is 16.23 g and 176.4 g, respectively.The number of moles of solute is calculated by the formula, n1 = m1/MW1Where,m1 is the given mass of solute MW1 is the molar mass of soluteSubstitute the given mass and molar mass in the above formula. n1 = 16.23g / MW1 The number of moles of diethylether is calculated by the formula, n2/MW2Where,m2 is the given mass of diethylether MW2 is the molar mass of diethylether Substitute the given mass and molar mass of chloroform in the above formula. n2 = 176.4 g /74.12 gmol-1 = 2.38 molWe make use of Raoult's law of relative lowering of vapour pressure and calculate molar mass of the Solute.(P° -Psolution) /P° = n1/n2Putting values ;(463.57-452.86)/463.57 = 16.23g /2.38 mol * MW1= 295.2 g/molHence, molar mass of the solute is found to be;295.2 gmol-1