
A mixture of CH4(g) at 0.500 atm and O2(g) at 0.750 atm is present in a 3.00L container at 28°C. The mixture is ignited by a spark and reacts according to the equation provided below. What is the total pressure in the container, now at 44°C, after the

The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases. a) What is the mole fraction of each gas in the mixture? b) If the mixture occupies a volume of 11.5 L at 65 degress C, calculate the total number of

A bearthing mixture used by deepsea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1.2 atm if PHe = 0.98 atm and PCO2 = 0.04 atm? a) 1.02 atm b) 0.12 atm c) 0.94 atm d) 0.18 atm

Consider the reaction 3CH4(g)= C3H8(g)+ 2H2(g).Calculate Delta G at 298 K if the reaction mixture consists of 40 atm of CH4 , 0.011 atm of C3H8, and 2.1×10−2 atm of H2.

Consider the reaction 3CH4(g)= C3H8(g)+ 2H2(g).Calculate Delta G at 298 K if the reaction mixture consists of 40 atm of CH4 , 0.011 atm of C3H8, and 2.1×10−2 atm of H2.


Consider the reaction: SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After

3CH4(g)>C3H8(g)+2H2(g) Calculate change in G at 298 k if the reaction mixture consists of 41atm of CH4 , 0.010 atm of CH3, and 2.3×10−2 atm of H2.

Four gases were combined in a gas cylinder with these partial pressures: 3.5 atm N2, 2.8 atm O2, 0.25 atm Ar, and 0.15 atm He.What is the mole fraction of N2 in the mixture?

A 10.00g sample of a mixture of CH4 and C2H4react with O2 at 25C and 1 atm to produce CO2 and water. If the reaction produces 520kJ of heat what is the mass percent of CH4 in the mixture? I don't want the answer just how to o

A 10.0 gram sample of a mixture of CH4 and C2H4 reacts with oxygen at 25°C and 1 atm to product carbon dioxide gas and liquid water. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture? PLEASE HELP! I do not know

The gases in a mixture have the following partial pressures at the same volume and temperature: 1,013,000 Pa nitrogen, 700. mmHg argon, 1.20 atm of helium, 790. torr oxygen, and 0.50 atm of carbon dioxide. What is the total pressure of the mixture in atm?

Consider the following reaction: H2+I2<>2HI A reaction mixture at equilibrium at 175 K contains P(H2)=0.958 atm, P(I2)=0.877 atm, and P(HI)=0.020 atm. A second reaction mixture, also at 175 K, contains P(H2)=P(I2)=0.616 atm, and P(HI)=0.106 atm.

A 10.0 gram sample of a mixture of CH4 and C2H4 reacts with oxygen at 25°C and 1 atm to product carbon dioxide gas and liquid water. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture? I am all out of tries on the

The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.46 atm at 500 K. PPCl5 =

At 750°C, the Kp for the reaction 2 CO + O2➞ 2 CO2 is 2.72 x 10^11. ( 2.72 times ten to the eleventh) At that temperature, CO and O2 are added to a constant volume vessel. The initial pressure of the CO is 2.00 atm, and that of the O2 is 1.50 atm.


A gas mixture containing N2 and O2 was kept inside a 2 L container at a temperature of 23 C and a total pressure of 1 atm. The partial pressure of oxygen was .722 atm. How many grams of nitrogen were present in the gas mixture?

A mixture of Xe, Kr, and Ar has a total pressure of 6.7 atm. What is the mole fraction of Kr if the partial pressures of XE and Ar are 1.6 atm and 2.8 atm? Did anyone get .343 ?

please can someone help me with these questions? 24) Which represents the largest pressure? A) five mm Hg B) one atmosphere C) one millimeter of mercury D) one hundred pascals E) five pounds per square inch 25) What would be the new pressure if a 400 mL

1. A cylinder of Xenon has a volume of 750. ml. At 25.0°C the cylinder has a pressure of 655 torr. How much Argon is present in the cylinder? a. 240. moles b. 0.0264 moles c. .315 moles d. 26.5 moles 2.If a 25 liter cylinder of gaseous ammonia at

CH4(g) + 2O2(g) = CO2(g) + 2H20(g). What volume of O2 is required to react with 2.0 mol CH4 at 50 degrees Celsius and .500 atm?

a gaseous mixture contains 1 mol of O2 and 2 mol of CO2, exerting a total pressure of 1.5 atm. what amount of CH4 must be added to the mixture in order to increase the total pressure to 2 atm. (assume no gas escapes and there is no change in total volume)

Given the initial concentrations of 0.10 atm NO2 and 0.10 atm N2O4 in a 1.0 L flask, what will be the equilibrium partial pressure of NO2? N2O4(g)=2NO2 Kp=0.660at319K Choose one answer. a. 0.10 atm b. 0.31 atm c. 0.045 atm d. 0.72 atm e. 0.19 atm

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00L vessel the equilibrium mixture contains 1.15 g of SO3 and 0.107 g of O2. 1) How many grams of SO2 are in the vessel?  A flask is charged with 1.500 atm of N2O4(g)

What is the total pressure of a mixture of 0.3 atm of F2, 0.5 atm of Cl2, and 0.8 atm of O2?

CO(g) + 2H2(g) ↔ CH3OH(g) Kc=14.5 (500K) a. In which direction will the reaction proceed if the reaction vessel contains 0.500 atm CO, 0.500 atm H2, and 0.500 atm CH3OH? Show your calculations for full credit. Remember that Q and K both have to be


At 750°C, the Kp for the reaction 2 CO + O2➞ 2 CO2 is 2.72 x 10^11. ( 2.72 times ten to the eleventh) At that temperature, CO and O2 are added to a constant volume vessel. The initial pressure of the CO is 2.00 atm, and that of the O2 is 1.50 atm.

In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is ________ if the partial pressures of He and Ne are 1.50 and 2.00 atm respectively. pHe = 1.50 atm. pNe = 2.00 atm. pAr = 8.40 atm  1.50  2.00 = ?? mole

A sample of argon at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0. °C. What is the new pressure? 105 atm 45.5 atm 54.9 atm 23.8 atm 42.7 atm

A 75.0 L stainless steel container was charged with 3.00 atm of hydrogen gas and 4.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at 25°C? in atm What is the pressure in the tank at 125°C? in atm

Consider the conditions listed in the table below. Gas Temperature Pressure H2 100 oC 1 atm CH4 100 oC 20 atm O2 373 K 1 atm CO2 373 K 10 atm Which describes the characteristics of these samples? I. All molecules have the same kinetic energy II. The

How many milligrams of a mixture containing equal numbers of moles of CH4 and N2 at 10 ATM total pressure will dissolve in 1 L of water at 20°C ??? Convert 16g/mol CH4 28g/mol N2 ???need density .998g/ml H2O

Consider the reaction: 2 H2S(g)>< 2H2(g) + S2 Kp= 2.4 x 10^4 at 1073k A reaction mixture contains .112 atm of H2,.055 atm of S2, and .445 atm of H2S. Is the reaction mixture at equlibrium? If not, in what direction will the reaction proceed?

Consider the reaction: 2 H2S(g)>< 2H2(g) + S2 Kp= 2.4 x 10^4 at 1073k A reaction mixture contains .112 atm of H2,.055 atm of S2, and .445 atm of H2S. Is the reaction mixture at equlibrium? If not, in what direction will the reaction proceed?

A mixture of gases contains twice as many moles of As as Kr. If 0.300 mol of Xe is added to this mixture, the pressure increases from 1.26 atm to 1.47 atm. how many moles of Ar are in the mixture?

You are studying the formation of HI(g) from its gaseous elements H2(g) and I2(g). The free energy of formation of HI(g) is –10.10 kJ/mol at 500 K. When the free energy change of the process at 500 K is zero, the reaction mixture shows partial pressures


The Kp for the following equilibrium system is 4.31 x 10‒4 at 375°C : N2(g) + 3H2(g) ↔ 2NH3(g). If 0.862 atm of N2 and 0.373 atm of H2 were mixed in a constantvolume flask and heated to 375°C, which of the following would be closest to the

mole fraction is equal to partial pressure divided by the total pressure Total pressure= sum of partial pressure use PV=nRT where n= number of moles equation become PV/RT=n make sure to convert the temperature to Kelvin and to use 0.0821 for R. V=volume,

A mixture of methane and helium is placed in a 2.0 l flask at 27 degrees the partial pressure of methane is 0.72 ATM and the partial pressure of helium is 0.22 ATM . What is the mole fraction of ch4?

A gaseous mixture in a 25.00 L container is made of 16.0 g N2 and 14.0 g Ar and has a total pressure of 1.00 atm. 1.Calculate the partial pressure of the N2 in the mixture. the ans is 0.620 atm 2.Calculate the temperature of the gas mixture. can someone

the solubility of argon in water at 25 degrees celcius is 0.0150M. what is the henry's law constant of Ar if the partial pressure of argon is 0.00934 atm. A)0.000140 M/atm B)0.623 M/ atm C)1.61 M/atm D) 4.10 M/atm K=Pgas/Cgas Post your work if you get

A mixture of 1.39 g H2 and 1.60 g He is placed in a 1.00L container at 27°C. Calculate the partial pressure of each gas and the total pressure. PH2 = ? atm PHe = ? atm Ptotal = ? atm Please put answer so i can compare to my answer

Consider the reaction: SO2 (g) + NO2 (g) SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 If the reaction vessel is instead charged initially with SO3(g) and NO(g), each at a partial pressure

To increase the solubility of a gas at constant temperature from 1.20 g/L at 1.4atm to 2.3 g/L the pressure would have to be increased to ______ A. 0.37 atm B. 0.7 atm C. 1.37 atm D. 2.7 atm

A flask initially contains 2.00 atm of NH3, 2.00 atm of N2, and 3.00 atm of H2 at 673 Kelvin. What is the delta G for the reaction? What is the equilibrium partial pressures of each gas at 673 Kelvin? So I figured out how to do the first question with

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the balls on both sides). My


Hurricane Katrina, which hit the Gulf Coast of Louisiana and Mississippi on August 29, 2005, had the second lowest ever recorded barometric pressure at 920mb. Convert this pressure to units of atmospheres, and inches of Hg. 1 bar = 0.98692 atm 0.92 bar =

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the balls on both sides). My

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the balls on both sides). My

A mixture of ammonia and oxygen is prepared by combining 0.330 L of NH3 (measured at 0.790 atm and 22°C) with 0.210 L of O2 (measured at 0.820 atm and 48°C). How many milliliters of N2 (measured at 0.740 atm and 100. °C) could be formed if the following

A mixture og gases has a total pressure off 28.3 atm, it is made of: 5.8 atm of hydrogen gas, 7.2 atm of nitrogen gas, 3.5 atm of oxygen gas and some amount of methane. What is the pressure of methane? what is the pressure of methane in kPa?

Consider the following reaction: C(s) + H2O (g) ⇌ CO (g) + H2 (g) (Kp = 0.45 at 900 K) What is the equilibrium partial pressure of H2O when the initial partial pressure of water is 1.00 atm? a) 0.43 atm b) 0.58 atm c) 0.22 atm d) 0.52 atm e) 1.16 atm

The local weather forecaster reports that the current barometric pressure is 29.5 inches of mercury. What is the current pressure in atmospheres? 9.99 atm 3.93 atm 0.986 atm 883 atm 1.00 atm

3H2(g)+N2(g)=2NH3(g) Suppose the equilibrium constant Kp = 0.003337 for the reaction above. If the equilibrium mixture contains partial pressures H2 = 0.400 atm and N2 = 0.350 atm. What is the equilibrium partial pressure of NH3 in atm?

The reaction 2 H2S(g)> 2 H2(g) + S2(g) has Kp = 2.4 x 104 at 1073 K. A reaction mixture contains 0.146 atm of H2, 0.041 atm of S2 and 0.574 atm of H2S. What is the value of Qp?

What volume of NO measured at 1.1 atm and 1100 C, can be produced from 10.0 L of NH3 and excess O2 measured at the same temperature and pressure? Here is the balance equation 4NH3+3O2+4NO+6H20 So far this is what I have: (1.1 atm)(10.0L)


what is the total pressure of a gas mixture that contains hydrogen at 0.45atm nitrogen at 0.25 atm and argon at 0.60 atm

2.40 L of N2, at 25 ∘C and 1.89 atm , is mixed with 2.60 L of O2, at 25 ∘C and 0.245 atm , and the mixture allowed to react. N2(g)+O2(g)→2NO(g) How much NO, in grams, is produced?

What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm

What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm?

What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm

ii) What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm

A mixture of ammonia and oxygen is prepared by combining 0.330 L of NH3 (measured at 0.710 atm and 22°C) with 0.200 L of O2 (measured at 0.740 atm and 51°C). How many milliliters of N2 (measured at 0.740 atm and 100. °C) could be formed if the following

for the haber process for the synthesis of ammonia: N2(g)+ 3H2(g)= 2NH3(g), what is ΔG (kJ/mol) at298 K for a reaction mixture that consists of 1.5 atm N2,3 atm H2 and 1.8 atm NH3? [ΔG° f(NH3)= 16.66kJ/mol]

Whats total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm

Each of the following processes is spontaneous as described. Which one will have ∆H approximately equal to zero? 1. precipitating 1 mol of AgBr(s) from a solution of Ag+(aq) and Br−(aq) 2. 1 L He(1 atm, 298 K) + 1 L Ar(1 atm, 298 K) → 2 L


Use van der Waals’ equation to calculate the pressure exerted by 2.33 mol of ammo nia at −3.7◦C in a 1.25 L container. The van der Waals’ constants for ammonia are a = 4.00 L2·atm/mol2 and b = 0.0400 L/mol. (The values for a and b have

The volume of a scuba tank is 10.0L.It containes a mixture of nitrogen and oxygen at 290.atm.what volume of this mixture could the tank supply to a diver at 2:40 atm?

At 58.8 degrees C and at a total pressure of 1.00 atm the mole percent of acetone in the vapor state above a solution of acetone and water containing 70. mol % acetone is 87.5%. Assuming the solution to obey Raoult's Law, determine the vapor pressure of

A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250 mole O2 , and an unknown quantity of He. The temperature of the mixture is 0 ∘C , and the total pressure is 1.00 atm . How many grams of helium are present in the gas mixture?

A sample of gas with a volume of 2.0 L exerts a pressure of 1.0 atm. If the volume is changed to 1.0 L (at constant temperature), what is the pressure? a. 0.5 atm b. 1.0 atm c. 2.0 atm d. 4.0 atm

A sample of krypton gas occupies 95.0 mL at 0.500 atm. If the temperature remained constant, what volume would the krypton occupy at (a) 5.00 atm, (b) 0.0500 atm, (c) 555 torr, (d) 5.00 torr, and (e) 5.5 3 1022 torr?

An aqueous solution is composed of 7.50 g NaCl (MM = 58.44 g/mol) diluted to 0.100 L. Calculate the osmotic pressure of the solution at 298 K a. 5.83 atm b. 9.22 atm c. 18.3 atm d. 62.8 atm

At 25 °C, the equilibrium partial pressures for the following reaction were found to be PA = 6.30 atm, PB = 7.20 atm, PC = 6.40 atm, and PD = 9.10 atm. 2A(g) + 2B(g)>C(g) + 3D(g) What is the standard change in Gibbs free energy of this reaction at 25

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the

A mixture containing 2.81 g each of CH4 (g), C2H4 (g) and C4H10 (g) is contained in a 1.50 L flask at a temperature of 35 oC. What is the partial pressure (in atm) of C4H10 (g)?


17 liters of a gas is at an initial temperature of 67 degrees C and a pressure of 88.89 atm, what will be the pressure of the gas if the tempetature of the gas is raised to 94 degrees C and the volume of the gas is decreased to 12 liters? 177 atm 36.3 atm

Is the answer for part c 0.91? A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill

The gase in a mixture have the following partial pressures at the same volume and temperature, 1013000Pa nitrogen, 700mm argon, 1.20atm helium, 790 torr oxygen, and 0.50 atm of carbon dioxide. What is the total pressure of tyhe mixture in atm? You add

The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.200 atm of oxygen and a total pressure of 3.00 atm, calculate the mass of helium in 10.0 L of the gas mixture at 40 degrees Celsius.

150.0 mL flask contains 740. g of N2 at 0°C. What is the pressure in atm. What is the pressure in torr? What is the pressure in psi? I know you have to do: n = grams/molar mass Then PV = nRT R in 0.08206 L.atm/mol.K gives P in atm atm x 760 = p in torr 1

Convert 3.6 times 10 to the second atm to torr. I don't understand how to get atm to torr???? 1 atm = 760 torr. Is the answer 270,000 torr? Are you in to significant figures. I suspect so since the question is 3.6 x 10^2 atm. If so, then 3.6 x 10^2 atm x

The pressure in a constantvolume gas thermometer is 0.700 atm at 100°C and 0.512 atm at 0°C. (a) What is the temperature when the pressure is 0.0500 atm? °C (b) What is the pressure at 405°C? atm

If 3.50 mol of A is mixed with 0.750 mol of B and the final pressure of the mixture is 3.25 atm, what are the partial pressures of A and B

A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800C. Calculate the equilibrium partial pressures of H2 Cl2 and HCl if the total pressure is 2.00 atm. For the reaction Kp is 193 at 2800C. H2(g) +Cl2(g) = 2HCl (g) What I've done so far:

4.80 L of N2, at 25 ∘C and 1.22 atm , is mixed with 1.80 L of O2, at 25 ∘C and 0.122 atm , and the mixture allowed to react. N2(g)+O2(g)→2NO(g) How much NO, in grams, is produced?


A snorkeler takes a syringe filled with 16 mL of air from the surface, where the pressure is 1.0 ATM, to an unknown depth. The volume of the air in the syringe at this depth is 7.5 mL. What Is the pressure at this depth? If the pressure increases by an

Use the PV diagram of a system. The units for P and V are atmospheric pressure atm and liter L. Process A to B and B to C are straight lines on it. How much is the work done by the system from A to C in J? Given these coordinates:(volume on the x, pressure

Fluorine and krypton react to form binary compounds when a mixture of the two gases is heated to 500C in a nickel reaction vessel. A 100mL nickel container is filled with fluorin and krypton to partial pressures of 1.24 atm and 10.10 atm, respectively at a

A gas occupies a volume of 0.500L at 125 degrees Celsius and 0.443 atm. What mathematical expression will yield the correct temperature at 0.750 L and 0.689 atm? Is it the combined gas law of P2V1/T1=P2V2/T2?

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the

Most natural gas consists of about 90% methane, CH4. Assume that the solubility of natural gas at 20 C and 1 atm gas pressure is about the same as that of CH4, 0.02 g/kg water. If a sample of natural gas under a pressure of 20 atm is kept in contact with

Triple Point Clicker Challenge The Lewis structure for nitroglycerin is shown below. 1.00 mL of liquid nitroglycerin is placed in a sealed, reinforced, insulated steel box measuring 1.00 m on each side and filled with argon gas at 15.0 oC and 1.00 atm. The

I've been trying to do this problem but I would get confused and stuck.. Consider a sample of a hydrocarbon at 0.959 atm and 298 K. Upon combustion the entire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 1.51 atm and

A rigid cylinder contains a sample of gas at STP. What is the pressure of this gas after the sample is heated to 410 K? a. 1.0 atm b. 0.50 atm c. 0.67 atm d. 1.5 atm Explain how you get the answer.

What pressure would a mixture of 3.2 grams of O2, 6.4 grams CH4, and 6.4 grams of SO2 exert if the gases were placed in a 5.1 liter container at 127C? Answer in units of atm


Find the mass of each of the following: (a) 5.52 L O2 at 1.89 atm and 250.0 K (b) 3.43 L NH3 at 0.911 atm and 27°C (c) 117 mL SO2 at 0.823 atm and 53°C

A XXg sample of methane, CH4, is mixed with YY atm of O2 (an excess) in a VV L combustion chamber at 125.0°C. The combustion reaction to CO2 and H2O is initiated and the vessel is cooled back to 125.0°C. What is the final pressure in the combustion

calculate the Henry's law proportionality constant for N2? partial pressure at 1 atm=0.78 atm solubility at 1 atm= 5.3 x 10^3 mol/L

calculate the Henry's law proportionality constant for N2? partial pressure at 1 atm=0.78 atm solubility at 1 atm= 5.3 x 10^3 mol/L

What pressure would a mixture of 3.2 grams of O2, 6.4 grams CH4, and 6.4 grams of SO2 exert if the gases were placed in a 4.1 liter container at 127 degrees C? Answer in units of atm