Calculate the molecular weight when a gas at 25.0 ∘c and 752 mmhg has a density of 1.053 g/l .

26.0 g/mol The ideal gas law is PV = nRT where P = pressure V = volume n = amount of substance R = ideal gas constant (8.3144598 (L kPa)/(K mol) ) T = absolute temperature Solving for n, gives PV = nRT PV/RT = n Convert pressure from mmHg to kPa 752 mmHg = 752 * 0.133322387415 = 100.2584353 kPa Convert temperature from C to K 25.0 C = 25.0 C + 273.15 = 298.15 K Volume will be 1 liter. Substitute known values into equation solving n PV/RT = n (100.2584353 kPa * 1 L)/(8.3144598 (L kPa)/(K mol) 298.15 K) = n (100.2584353 kPa L)/(2478.956189 (L kPa)/mol) = n 0.040443811 mol = n So we know we have 0.040443811 moles of the unknown gas. Now just divide the mass of the gas by the number of moles. 1.053 g / 0.040443811 mol = 26.03612214 g/mol Rounding to 3 significant figures give 26.0 g/mol

A. 17 hope this dudet

Because electrons have negligible mass, to account for the mass of the isotope, there must be 16 neutrons, 16 neutrally charged, massive, fundamental particles present in the sulfur nucleus. and thus finally, if we have the 32s2− ion, there are 18 electrons, 16 protons, and 16 neutrons.