The vapor pressure of CCl3FCCl3F at 300 KK is 856 torr. |
Part A If 11.5 gg of CCl3FCCl3F is enclosed in a 1.1 LL container, calculate the number of moles of CCl3FCCl3F in the gas phase. Express your answer using two significant figures.
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The vapor pressure of CCl3FCCl3F at 300 KK is 856 torr. Part A If 11.5 gg...
The vapor pressure of CCl3F at 300 K is 856 torr. If 11.0 g of CCl3F is enclosed in a 1.2 L container, calculate the number of moles of CCl3F in the gas phase. Express your answer using two significant figures.
I need help with question or Part C and if you could please write it out so i can understand it? The rest of the question is attached as i know you need to know the rest of the information to anwser the question.... The vapor pressure of CCl3F at 300 K is 856 torr. Part A If 11.5 gg of CCl3FCCl3F is enclosed in a 1.1 LL container, calculate the number of moles of CCl3FCCl3F in the gas phase....
Part C Taking into account the vapor pressure of water, how many moles of hydrogen gas, n, are present in 311 mL at 752 torr and 29 °C?The value of the gas constant Ris 0.08206 L-atm/(mol-K). You may also find the conversion factors 1 atm = 760 torr and Tk = Te + 273 useful. Express the number of moles to three significant figures. View Available Hint(s) 190 AED ? mol Submit
Part A A sample of hydrogen gas is mixed with water vapor The mixture has a total pressure of 759 torr, and the water vapor has a partial pressure of 26 torr What amount (in moles) of hydrogen gas is contained in 1.73 L of this mixture at 298 K? Express the amount in moles to three significant figures. O ALO O 2 ? amount = mol Submit Request Answer
Taking into account the vapor pressure of water, how many moles of hydrogen gas, n, are present in 343 mL at 752 torr and 29 ∘C?The value of the gas constant R is 0.08206 L⋅atm/(mol⋅K). You may also find the conversion factors 1 atm=760 torr and TK=TC+273 useful. Express the number of moles to three significant figures.
The vapor pressure of trichloromethane (chloroform) is 41.5 Torr at -7.6 ∘C. Its enthalpy of vaporization is 29.2 kJ⋅mol−1. Calculate its normal boiling point. Express your answer using three significant figures.
The vapor pressure of ethanol (C2H5OH) at 19 ∘C is 40.0 torr. A 1.10 g sample of ethanol is placed in a 2.60 L container at 19 ∘C. If the container is closed and the ethanol is allowed to reach equilibrium with its vapor, how many grams of liquid ethanol remain?Express your answer to two significant figures and include the appropriate units.
The vapor pressure of a liquid is 300 torr at 51.0 °C, and its enthalpy of vaporization is 37.66 kJ/mol. Calculate the normal boiling point of this liquid in °C?
Part A Calculate the volume of the gas, in liters, if 1.60 mol has a pressure of 1.20 atm at a temperature of -5 ∘C. Express the volume in liters to three significant digits. V V = nothing L SubmitRequest Answer Part B Calculate the absolute temperature of the gas at which 3.53×10−3 mol occupies 478 mL at 760 torr . Express the temperature in kelvins to three significant digits. T T = nothing K SubmitRequest Answer Part C Calculate...
Part (A) What is the calculation using the molar volume for each of the following at STP? Express your answer with the appropriate units. 1) the number of moles of O2O2 in 39.0 LL of O2O2 gas 2) the volume, in liters, occupied by 2.99 moles of N2N2 gas 3) the volume, in liters, occupied by 54.5 gg of ArAr gas 4) the number of grams of H2H2 in 1420 mLmL of H2H2 gas Part (B) A sample of neon...