The vapor pressure of water at 25.0°c is 23.8 torr. determine the mass of glucose (molar mass = 180 g/mol) needed to add to 500.
0 g of water to change the vapor pressure to 22.8 torr.42.a solution is prepared from 53.8 g of a nonvolatile, nondissociating solute and 85.0 g of water. the vapor pressure of the solution at 60°c is 132 torr. the vapor pressure of water at 60°c is 150. torr. what is the molar mass of the solute?ans:epts:1dif:difficultref:11.4chemistry | general chemistry | solutions | colligative properties | vapor pressure of a solution | vapor pressure loweringmsc: quantitative43.an ideal solution is formed from a mixture of the nonvolatile solute urea, co(nh2)2, and methanol, ch3oh. the vapor pressure of pure methanol at 20°c is 89 mmhg. if 4.4 g of urea is mixed with 39.9 g of methanol, calculate the vapor pressure of the methanol solution.a) 4.9 mmhgb)80 mmhgc)74 mmhgd) 15 mmhge)84 mmhg44.a salt solution sits in an open beaker. assuming constant temperature and pressure, the vapor pressure of the solution
Q: A according to this formula, we can get the mole fraction of water (n): P(solu) = n Pv(water) when we have Pv(solu) = 22.8 and Pv(water) = 23.8 so by substitution: 22.8 = n * 23.8 n= 0.958 - we need to get the moles of glucose: moles of water = 500 g(mass weight) / 18 (molar weight)= 27.7 mol n = moles of water / ( moles of water + moles of glucose) 0.958 = 27.7 / ( 27.7+ moles of glucose) 0.958 moles of glucose + 26.5 = 27.7 0.968 moles of glucose = 1.2 moles of glucose = 1.253 mol ∴ the mass of glucose = no.of glucose moles x molar mass = 1.253 x 180 = 225.5 g Q: B here we also need to get n (mole fraction of water )by using this formula: Pv(solu) = n Pv(water) when we have Pv(solu)=132 & Pv(water)=150 so, by substition: 132= n * 150 n = 0.88 so, mole fraction of solution = 1 - 0.88 = 0.12 and we can get after that the moles of water = (mass weight / molar mass) - no.moles of water = 85 g / 18 g/mol = 4.7 moles - total moles in solution = moles of water / moles fraction of water = 4.7 / 0.88 = 5.34 moles ∴ moles of the solution = total moles in solu - moles of water = 5.34 - 4.7 = 0.64 moles solute ∴ the molar mass of the solute = mass weight of solute / no.of moles of solute = 53.8 / 0.64 = 84 g/mole
Q: C
moles of urea (NH2)2 CO = mass weight / molar mass = 4.49 g / 60 g /mol = 0.07 mol moles of methanol = mass weight / molar mass = 39.9 g / 32 g/mol = 1.25 mol moles fraction of methanol = moles of methanol / (moles of methanol + moles of urea ) moles fraction of methanol = 1.25 / ( 1.25+0.07) = 0.95 by substitution in Pv formula we will be able to get the vapour pressure of the solu : Pv(solu) = n P°v Pv(solu) = 0.95 * 89 mm Hg ∴Pv(solu) = 84.55 mmHg
In large doses it stops cells using oxygen causing these cells to die. So in a small amount it would not kill you. So lets say cyanide is inside the body it would kill off all the cells and your body would not be able to function causing death
