
Calculate the volume at s.t.p. occupied by a gas 'Q' originally occupying 153.7cc at 287K and 750mm pressure [vapor pressure of at 287K is 12mm of Hg]

Calculate the volume at s.t.p. occupied by a gas 'Q' originally occupying 153.7cc at 287K and 750mm pressure [vapor pressure of gas 'Q'at 287K is 12mm of Hg]

Calculate the volume at s.t.p. occupied by a dry gas 'Q' originally occupying 153.7cc at 287K and 750mm pressure [vapor pressure of gas 'Q'at 287K is 12mm of Hg]

the volume at s.t.p. occupied by a gas q originally occupying 153.7 cc at 287 k and 750mm pressure, vapour pressure of gas q at 287k is 12 mm of hg

The volume at stp occuppied by a gas Q originally occupying 153.7dm at 287k and 750mm pressure (vapor pressure of gas Q at 287k is 12mm of Hg)


The volume at stp occuppied by a gas Q originally occupying 153.7dm at 287k and 750mm pressure (vapor pressure of gas Q at 287k is 12mm of Hg)

A gas occupying 29 mL at standard conditions is heated to 14◦C while the pressure is reduced to 0.98682 atm. What is the new volume occupied by the gas?

A gas occupying 43 mL at standard conditions is heated to 29 celsius while the pressure is reduced to 0.84091 atm. What is the new volume occupied by the gas?

A gas occupying 10 mL at standard conditions is heated to 10◦C while the pressure is reduced to 0.92114 atm. What is the new volume occupied by the gas? Answer in units of mL

It turns out that the Van Dar Waals constant b is equal to four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms: a) at STP b)

The pressure of a gas having volume 1800ml. Originally occupying 300ml. at 6 atms. Pressure.

It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of volume in a container actually ocupied by Ar atoms (a) at STP, (b) at 100

Calculate the volume occupied by 3moles of a gas at r.t.p

calculate the volume occupied by 30.5grams of ammonia gas at s.t.p. (N=14,H=1)

calculate the volume occupied by 7g of N2 gas at 27 degree c and 750mm Hg pressure


calculate the volume occupied by 10^22moleculesof a gas 300k and 760mm pressure

calculate the volume occupied by 10^22 molecules of a gas 300 k and 760 mm pressure. please help me please...................

Calculate the volume occupied by 7g of nitrogen gas at 27 degree c and 750 mm of hg pressure

A sample of a monatomic ideal gas is originally at 20 °C. Calculate its final temperature of the gas if the pressure is doubled and volume is reduced to onefourth its initial value.

A sample of a monatomic ideal gas is originally at 20 °C. Calculate its final temperature of the gas if the pressure is doubled and volume is reduced to onefourth its initial value.

Part B TrueFalse Classify each of the statements as always true, sometimes true, or never true. 1.____ST______ one mole of any gas occupies a volume of 22.4 L. 2_____NT______ for a substance of known molar mass, the number of moles of a sample can be

Calculate The Volume Occupied By 10(superscript)22 Molecule Of Gas At 300 kalvin And 760mm Pressure

the volume of a gas was originally 2.5 L; it's pressurewas 104kpa and its temperatire was 270K. the volume of the gas expanded to 5.3 L and its pressure decreased to 95 kpa. What is the temperature of the gas?

What is the volume occupied by 0.118mol of Helium gas at a pressure of 0.97atm and a temperature of 305k? Would the volume be different if the gas was Argon(under the same identical conditions)?

find the molar mass of 7.5gm of a gas occupying 5.8 lt volume at s.t.p.


Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 atm.

Find the pressure of a gas that originally had a volume of 25 L, pressure of 67kPa at a temperature of 100 Kelvin. When the gas was heated to 200 Kelvin, it had a volume of 56L. How many moles would be present if the gas in the above question was an ideal

calculate the pressure in atm of a balloon filled with 7.5g of helium gas if the baloons volume decreases to 7.5L suppose the balloons pressure and volume are originally 799 mmHg and 15L

Helium gas, He, at 22 degrees C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquidnitrogen temperature (197 degrees celcius). What is the equation?

use the molar volume of a gas to solve the following at STP: a. the number of moles of O2 in 44.8 L O2 gas. b. the number of moles of CO2 in 4.00L CO2 gas. c. the volume(L) of 6.40g O2. d. the volume(mL) occupied by 50.0g neon.

8.10L container holds a mixture of two gases at 45 °C. The partial pressures of gas A and gas B, respectively, are 0.153 atm and 0.882 atm. If 0.110 mol a third gas is added with no change in volume or temperature, what will the total pressure become?

The vapour density of a gas is 22.4 and mass is. 22.4grams.what is the volume occupied the gas at N .T .P ?

What volume of H2 gas, in mL, would be occupied by 0.00465 moles of H2 gas at a temperature of 0 °C and a pressure of 760 mmHg?

formula: 2Cl ==> Cl2 + 2e in one experiment, the volume of chlorine gas formed was 18cm3. i) calculate the amount, in moles, of chlorine gas in 18cm3.(the volume of 1 mol of a gas at room temperature and pressure is 24000) ii) calculate the quantity of

A gas occupying a volume of 664 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?


A gas sample occupying a volume of 88.7 mL at a pressure of O.917 atm is allowed to expand at constant temperature until its pressure reaches 0.335 atm. what is its final volume?

A gas occupying a volume of 806 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?

A gas occupying a volume of 664 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?

One mole of nirtogen at 273K occupying 10 litres (state 1) is to be expanded to a volume of 20 litres at 373K (state 2). An infinite number of paths from state 1 to state 2 are possible. Consider the following important paths: (a) The gas is expanded

how do you solve the ideal gas law when you are given the temperature in celcius instead of kelvin. Heres an example question. Calculate the volume occupied by 3.25 moles of carbon dioxide at 25degrees celcius and 750mm Hg.

A gas occupied a volume of 3.50 L at 27 degrees celcius and 400.0 mmHg. What is the new temperature if the pressure changes to 0.789 atm and the volume is decreased to 2.50 mL

This problem is from my chemistry book and I am having a little trouble with the intermediary steps: Barium metal crystallizes in a body centered cubic lattice (atoms at lattice points only) The unit cell edge length is 502 pm, and the density of the

A gas sample occupies a volume of 400.0ml at 298.15k at costant pressure. what is the final temperature when the volume occupied decreased by 39.0

If 8.00 moles of a monatomic ideal gas at a temperature of 260 are expanded isothermally from a volume of 1.08 to a volume of 4.14 .Calculate the work done by the gas.Calculate the heat flow into or out of the gas.If the number of moles is doubled, by what

What is the volume at STP, in liters, occupied by 26.4 g of F2 gas?


What is the volume at STP, in liters, occupied by 26.4 g of F2 gas?

A fixed amount of CH4 gas occupies a volume of 136 mL at a pressure of 567 mm Hg and a temperature of 19oC. What will be the volume, in mL, occupied by this sample of CH4 gas when the pressure is decreased to 421 mm Hg while holding the temperature

Calculate the Volume occupied by 1.5 moles of an ideal gas at 25 degrees Celsius and a pressure of 0.80 atm. (R= 0.08206 L atm/(mol*K). I've tried using the ideal gas law: PV=nRT but i can't seem to get where I am getting lost. V=(1.5mol)(0.08206 L

i reallly need help with combining the gas laws. here are a few questions i am struggling with if anyone could please help! 1. A steel container holds 750.L of O2 gas at STP. a) how many moles of O2 does the container hold? b)how many grams of O2 does the

what is the volume occupied by 2 moles of ammonia at s.t.p(1mole of gas at s.t.p=22.4)

What is the volume occupied by 0.738g of xenon gas at STP?

How much volume will be occupied by 2 mole CO2 gas at stp?

3. suppose a gas at STP. Calculate its pressure at 25 degrees celcius if volume remains unchanged 5. suppose 1.11 L of an unknown gas in a rigid container constant volume is cooled from 22 deg. C to 55 deg C. Calculate the new pressure of the gas 6.)

A gas containing sulfur and fluorine analyzed as 29 % sulfur. A 140 g sample of a gas occupied a volume of 50.1 L with a pressure of 478.80 torr at 296.00 K. Enter the molecular formula of the compound.

A gas containing sulfur and fluorine analyzed as 29 % sulfur. A 140 g sample of a gas occupied a volume of 50.1 L with a pressure of 478.80 torr at 296.00 K. Enter the molecular formula of the compound.


What is the volume occupied by 0.252mol of helium gas at 1.35atm and 305K ?

what volume will be occupied by 3.25mol of oxygen gas at 735mmhg and 25celcius?

vapour density of gas is 11.2 volume occupied by 22.4gms at STP?

Use molar volume to solve the following problems at STP. Find the volume mL occupied by 0.400 mole He. Find the number of grams of neon contained in 10.2 L Ne gas

What is the volume occupied by 12.3 g or argon gas at a pressure of 1.17 atm and a temperature of 455K?

What is the volume, in L, occupied by 3.260 moles of NO2 gas at STP conditions?

What is the volume occupied by 12.9 g of argon gas at a pressure of 1.30 atm and a temperature of 318 K ?

What is the volume occupied by 20.9g of argon gas at a pressure of 1.09atm and a temperature of 411K ?

A mixture of ethyne gas (C2H2) and methane gas (CH4) occupied a certain volume at a total pressure of 16.8 kPa. When the sample burned, the products were CO2 gas and H2O vapor. The CO2 was collected and its pressure found to be 25.2 kPa in the same volume

A certain mass of gas occupied 450cm cube at 25°c.At what temperature will it have it's volume reduced half


What is the volume, in L, occupied by 1.20 moles of C2H6 gas at a temperature of 125oC and at a pressure of 1.55 atm?

What volume in liters is occupied by 8.22 g of SO2 gas confined at a pressure of 1200.8 torr at 75.0*c?

What volume would be occupied by 100 g of oxygen gas at a pressure of 1.50 atm and a temp of 25 degrees C.

Temp  650 Pressure  690mm Hg mass  0.927g volume  194cm3 How do I calculate the volume of the gas? You have the volume, given. How do I calculate the volume at a different temperature?

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 10.5g of neon at STP.

What is the volume occupied by 12.3 g of argon gas at a pressure of 1.17 atm and a temperature of 455K? Would formula be V=T/P? 388.89 L?

What is the volume occupied by 20.2g NH3(g) at 25 degrees celsius and 752 mmHg? This is Ideal Gas Law.

I keep getting the last part of this question wrong. Strong base is dissolved in 765 mL of 0.200 M weak acid (Ka = 4.63 x 10^5) to make a buffer with a pH of 4.18. Assume that the volume remains constant when the base is added. HA(aq) + OH(aq) . H2O(l)

Calculate the enthalpy of atomization per unit volume for Rb. Express your answer in kJ/m3. Determine the volume (in mL) occupied at room temperature by 3.5e22 mercury (Hg) atoms in the liquid state.

A gas containing carbon and hydrogen analyzed as 85.6 % carbon and 14.4 % hydrogen. A 42.1 g sample of a gas occupied a volume of 7490 mL with a pressure of 2280.0 torr at 92 °C. Enter the molecular formula of the compound. Thanks.


1. Calculate the number of molecules in a deep breath of air whose volume is 2.15 L at body temperature, 36 degrees Celsius, and a pressure of 740 torr. 2.A fixed quantity of gas at 24 degrees Celsius exhibits a pressure of 740 torr and occupies a volume

I'm having trouble trying to figure out how to setup and solve these problems: 1) 2,600.0 mL of air is at 20.0C. What is the volume at 60.0C? 2) A gas occupies 900.0 mL at a temperasture of 27.0C. What is the volume at 132.0C? 3) What change in volume

From the ideal gas law, calculate the volume per helium atom in a litre of helium gas kept at room temperature and atmospheric pressure. Additionally, calculate the length of the side of a cube with this volume.

From the ideal gas law, calculate the volume per helium atom in a litre of helium gas kept at room temperature and atmospheric pressure. Additionally, calculate the length of the side of a cube with this volume.

Please tell me which Gas Law equation to use to figure out this problem... A helium balloon at 25°C, 1 atm, has a volume of 2.88 L. Additional helium is pumped into the balloon. It now contains 1.20 g of He and its new volume is 7.20 L. How many moles of

Assuming that the temperature and quantity of a gas sample remain constant, what will be the final pressure of 1.6 L sample of gas originally at 330K and 4.84 atm, when the volume is reduced to 840 mL?

A sample of 8.02×10^−1 moles of nitrogen gas (γ =1 .40) occupies a volume of 2.00×10^−2 m^3 at a pressure of 1.00×10^5 Pa and temperature of 300K. The sample is isothermally compressed to exactly half its original volume. Nitrogen behaves as an

Please!!! its extremely urgent. i do not need answers, only how to do it A sample of nitrogen gas (N2) kept in a container of volume 10.1 L and at a temperature of 20.3°C exerts a pressure of 3.1 atm. Calculate the number of grams of gas present. Round to

1. Calculate the work done on the system when 1.00 mol of gas held behind a piston expands irreversibly from volume of 1.00dm cube to a volume 10.00dm cube against an external pressure of 1.00 bar. 2. A perfect gas expand reversibly at a constant

26 g of methane CH4 has a pressure of 450 kPa at 250 degrees celcius find the volume occupied by the gas


Find the volume occupied by 3.14 moles of an ideal gas at standard conditions of pressure and temperature (P = 1.00 atm, T = 273 K).

A 0.05 N solution of a salt occupying a volume between two platinum electrodes seprated by a distance of 1.72 cm an having an area of 4.5 cm2 has a resistance of 250 ohm. calculate equivalent conductance of a solution

A gas at 250K and 15atm has a molar volume smaller than calculated from perfect gas law Calculate: a) the compression factor under these conditions b) the molar volume of gas

I don't really know how to go about this, Please help 1. Calculate the number of moles of the gas. Calculate the volume the gas would occupy at 100.0 C and 15.0 atm. 10.8 g He 2. Given the volume of 54.0 C and 790 torr, calculate the number of moles and

Calculate The volume occupied at s.t.p by 0.24g of ozone ( o=16, G.M.V=22.4dm3

Calculate the volume occupied by 5.25 g of nitrogen at 26*c [temperature] and 74.2 cm of pressure.?

a flexible container at an initial volume of 7.14L contains 9.51mol of gas. more gas is then added to the container until it reaches final volume of 17.1L. assuming the pressure and temperature of the gas remain constant, calculate the number of moles of

A flexible container at an initial volume of 4.11 L contains 7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 15.9 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles

A flexible container at an initial volume of 8.15 L contains 2.51 mol of gas. More gas is then added to the container until it reaches a final volume of 12.1 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles

A flexible container at an initial volume of 5.12 L contains 7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 18.3 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles


A sample gas is 3.7 L at 15.3 degrees C and the pressure is held at constant. What would be the volume if the temp was raised to 153 degrees C?

An ideal gas originally at 0.8 atm and 77C was allowed to expand untel its final volume ,pressure and temperature were 600 ml ,0.4 atm and 27C.what was the initial volume

The temperature of an ideal gas in a 5.00 L container originally at 1.01 bar pressure and 25 °C is lowered to 220 K. Calculate the new pressure of the gas.

At 650 degree C and a pressure of 690mm HG, the 0.927g sample has a volume of 194cm3. How do I calculate the volume at the same temp but at a pressure of 760mm Hg? Also, how do I calculate the volume at the same pressure but at a temp of 0 degree C? Thanks

if you have a gas sample that has a mass of .993g occupying .570L. Given the temperature is 281K and the pressuere is 1.44 atm, what is the molar mass of the gas?