Propane, C3H8, liquefies under modest pressure, allowinga large amount to be stored in a container. (a) Calculatethe number of moles of propane gas in a 110-L container at3.00 atm and 27 °C. (b) Calculate the number of moles ofliquid propane that can be stored in the same volume if thedensity of the liquid is 0.590 g/mL. (c) Calculate the ratioof the number of moles of liquid to moles of gas. Discussthis ratio in light of the kinetic-molecular theory of gases.

For many purposes we can treat butane (C4H₁0) as an ideal gas at temperatures above its boiling point of -1. °C. Suppose the pressure on a 86.0 g sample of butane gas at 15.0°C is reduced to one-third its initial value. Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. O yes O no 0.P X

What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's engine upon consumption of a 62.0 L LIQUID tank gasoline? (Gasoline density: 0.770 kg/L, Molar mass of C₈H₁₈: 114.2 g/mol) C₈H₁₈ (l) + ²⁵/₂ O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)

Given the following reaction, CaH2 (s) + H20 (1) ---> Ca(OH)2 (aq) + H2 (g) a) Balance the equation; b) How many moles of CaH2 are needed to generate 10.0L of H2 gas if the pressure of H2 is 740.0 mm Hg at 23.0 °C?

A 1,365.8 mL aqueous solution of 407.9 mM Na2S is combined with 100.0 mL of an aqueous HCl solution whose HCl concentration is not known. The reaction produces 3.36 L of H2S gas at a pressure of 1.00 atm and a temperature of 11.88∘C. There is some Na2S remaining after the reaction is complete. What is the concentration of sulfide ions in the solution after the reaction has completed? Assume the volumes of the solutions are additive. Express your answer in units of millimolar (mM) using at least three significant digits.

Air is 78.08% nitrogen; thus, when the atmospheric pressure is 1.00 atm the partial pressure of nitrogen, N2, is 0.7808 atm. How many molecules of nitrogen are there in a 1.00-L container of air at a total atmospheric pressure of 0.985 atm and a temperature of 25 degrees Celcius?

What is the pressure (in bar) of a 4.50 L tank with 2.00 moles of oxygen at 39.3 °C? R= 0.08314 L·bar/mol· K.

Consider the reaction: Li2O(aq) + CO2(g) Lİ2CO3(s) ----> What volume of cabon dioxide will react completely with 1.00 g of lithium oxide (Li20; 29.88 g/mol) at 25 °C and 1.00 atm?

A mixture of He, Ne and Ar has a pressure of 7.85 atm. If the Ne has a mole fraction of 0.47 and Ar has a mole fraction of 0.23, what is the partial pressure of He?

What is the equivalent pressure of 0.900 atm in units of mm Hg?