MOLES

The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???PV=nRT where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?.P. ?=P=     What is the pressure of 0.638 moles0.638 moles of an ideal gas at a temperature of 297.0 K297.0 K and a volume of 5.58 L?5.58 L? ?=P=   atm

A gaseous compound of phosphorus (P) and fluorine (F) was found to have a density of 3.50 g L' at a temperature of 25.0 °C and a pressurc of 740 tor. It was also found to consist of 35.2% P and 64.8% F in a volume of 1 L. Assume that the mass of the sample is 100.0 g. Determine a) (i) its empirical formula (ii) its molecular mass using its empirical formula stated in part (i) (iii) its molecular mass using ideal gas law (iv) its molecular formula. Explain why the molecular formula is same as empirical formula. Given that the molecular mass of P is 30.97 g mol'; the molecular mass of F is 19 g mol'; 1 atm = 760 torr

In a mixture of three gases (A, B, and C), the number of moles of each gas is known (nA, nB, and nC).  How would the mole fraction of gas A (χA) be calculated using the values nA, nB, and nC?

A cylinder of volume 27.0 L is filled with 25.1 g of jobstium gas (MM = 72.21 g · mol-1) from the planet Randomite at a temperature of 326 K. • Part A Determine the number of moles of jobstium gas present. Express your answer using three significant figures n= 0.348 mol Submit Previous Answers Completed Part B The cylinder contains 0.348 mol of jobstium under these conditions. What is the pressure in the cylinder (in bar)? Express your answer in bar to three significant figures. P = bar

Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutionsThe solutions should be : 3,92 g; 78,4%; 0,72 atm.I just dont know how to do it

Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutions

Part A. Multiple Choice Identify the choice that best completes the statement or answers the question. L·atm R = 0.08206 mol · K 1. At 0.982 atm, the height of mercury in a barometer is 0.746 m. If the mercury were replaced with ethanol, what height of ethanol (in meters) would be supported at this pressure? The densities of Hg and ethanol are 13.5 g/cm³ and 0.789 g/cm³, respectively. а. 0.0436 m b. 0.946 m с. 0.760 m d. 12.8 m е. 13.0 m

江苏高考分数线 A Acellus Applications of the Ideal Gas Law 0.0453 moles of hydrogen gas were produced by the reaction. Calculate the volume of the gas at standard temperature and pressure. Mg + 2HCI → MgCl2 + H₂ Volume H₂ = [?]L C Liters of H₂ Enter 28 2 Resources Help

Solid ammonium chloride, NH,Cl, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH; (g)+HCl(g) NH, CI(s) A 6.75 g sample of NH, gas and a 6.75 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C. Identify the limiting reagent. NH,C1 HCl NH, How many grams of NH, Cl will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,Cl produced by the reaction. P = atm

At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropane

The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as PV = nRT where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. Rearrange the equation to solve for T. T = What is the temperature of 0.574 mol of an ideal gas with a volume of 8.64 Land a pressure of 1.919 atm? T = K

Earth's atmosphere is approximately 78.0% nitrogen and 21.0% oxygen. What is the mass in grams of oxygen in a cubic meter of air in a typical classroom at 1 atm and 25° C? ( 1 m³ = 1000 L)

At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H) was burned, producing 18.7 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropane =

[References] A steel cylinder contains 5.00 moles graphite (pure carbon) and 5.00 moles O2. The mixture is ignited and all the graphite reacts. Combustion produces a mixture of CO gas and CO2 gas. After the cylinder has cooled to its original temperature, it is found that the pressure of the cylinder has increased by 40.0%. Calculate the mole fractions of CO, CO2, and O2 in the final gaseous mixture. Mole fraction of CO = Mole fraction of CO2 Mole fraction of O2 = Submit Answer Try Another Version 3 item attempts remaining Visited

The ideal gas law describes the relationship between pressure (P), temperature (T), volume (V), and the number of moles of gas (n). PV = nRT The additional symbol, R, represents the ideal gas constant. The ideal gas law is a good approximation of the behavior of gases when the pressure is low and the temperature is high. (What constitutes low pressure and high temperature varies with different gases.) In 1873, Johannes Diderik van der Waals proposed a modified version of the ideal gas law that better models the behavior of real gases over a wider range of temperature and pressure. na P + ")(v – nb) = nRT In this equation the additional variables a and b represent values characteristic of individual gases.

What is the mole fraction of 4.43 m KBr (aq)? Keep extra sig figs as you work this problem. Round to 3 significant figures at the end.

For molar masses, use 35.45 for chlorine and 1.008 for hydrogen. It will make a difference if you use a periodic table that has different ones. Assuming ideal behaviour, calculate the pressure in atmospheres of 2.19 kilograms of hydrogen chloride gas (HCl(g) - yes, hydrochloric acid is also called hydrogen chloride, and it's a gas at room temperature.  It's "liquid" when you use it in the lab because you use it dissolved in water!) in a 25.0 L container at 18°C.   a. 0.0574 atm b. 5814.5 atm c. 3.550 atm d. 57.4 atm e. 359.7 atm f. 5.81 atm

A 25lb bag of calcium chloride ice melt weighs 11.34kg . How many moles are in CaCl2?

Ideal Gas Law Fermentation of glucose produces gas in the form of carbon dioxide, how many moles of carbon dioxide are produced if 785 ml of carbon dioxide at 20.1°C and 90 kPa was collected during the process?   where V = volume in liters  P = pressure in atmosphere n = moles  T=temperature in Kelvin R= universal gas constant,    =0.0821 L atm/mol. K      =8.314 L kPa/mol, K