Search: a sample of gas has a volume of 1.00 l at STP What is the temp in C if the volume is 10.0 L at 2.00 atm

how many mmhg in 1 atm

Number of results: 28,093

a sample of helium gas is in a closed system with a movable piston. the volume of the gas sample is changed when both the temperature and the pressure of the sample are increased. the table below shows the initial temperature, pressure, and volume of the gas sample, as well as.

The pressure exerted on a 240. mL sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?

The pressure exerted on a 240.0 mL sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?

A sample of oxygen at room temperature occupies a volume of 5.00x102 mL at 1.50 atm pressure. What pressure (in atm) must be applied to compress the gas to a volume of only 1.50x102 mL? Assume the temperature is constant.

7.75 litres of radon gas is at 1.55 atm and -19 degrees c what is the volume at stp

what is the volume occupied by 0.118 mol of helium gas at a pressure of 0.97 atm & temp of 32 C? R= 0.0821 L atm/mol K

A sample of gas has a volume of 8.1 liters at 1 atmosphere pressure and 203.0 K. What is its volume (liters) at STP?

A sample of a gas at 0.73 atm occupies a volume of 245 mL. If the temperature remains constant, what will be the new pressure if the volume increases to 633 mL?

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?

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 of 4.42 L. a)Use Boyle.

A sample containing 6.40 g O2 gas has a volume of 15.0 L. Pressure and temperature remain constant. a. What is the new volume if 0.600 mole O2 gas is added? b. Oxygen is released until the volume is 12.0L. How many moles of O2 are removed? c. What is the volume after 7.50 g He.

a sample of natural gas at stp is 78% ch4 and 22% c2h6 by volume. how many moles of each gas are presented in 2 L of the mixture.assume ideal gas behavior

A sample of nitrogen (N2) gas has a volume of 250ml at 30 degrees C and a pressure of 745mmHg. What is the volume of the nitrogen at STP? I got 22 liters in significant figures is this right. thank you.

A sample of gas occupies a volume of 500.0mL at .906 atm and 97 C. What will the final temperature (in Celsius) be if it is brought to a volume of 1.05L and a pressure of 502 mm Hg?

A gas occupies 21.0 L at 2.00 atm pressure and 27oC. Calculate its volume at STP.

Part B True-False 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 calculated from the mass.

A sample of natural gas at STP is 78% CH4 and 22% C2H6 by volume. How many moles of each gas are present in 1.60L of the mixture? Assume ideal gas behavior

The volume of a sample of ideal gas at 25*C is 372ml. What will be the volume of the gas if it is heated at constant pressure to 50*C? What will be the volume of the gas if it is cooled to -272*C?

A sample of gas has an initial volume of 14.7L at a pressure of 1.02 atm. If the sample is compressed to a volume of 10.2L, what will its pressure be?

a sample of unknown gas is found to have a volume of 479 mL at 27.0 degrees C and 1.30 atm. How may moles of gas are int eh sample?

a sample of oxygen gas has a volume of 7.64 L at a temperature of 19C and a pressure of 1.38 atm. Calculate the moles of O2 present in this gas sample

a gaseous sample occupies 32.4 mL at -23 degrees C and 0.75 atm. What volume will it occupy at STP?

At 16°C a sample of ammonia gas exerts a pressure of 11.7 atm. What is the pressure when the volume of the gas is reduced to one-fourth of the original value at the same temperature so the inital Temp=16 C initial Pressure. 11.7 final pressure-unknown temperature-same what next?

sample of argon gas collected at a pressure of 1.11 atm and a temperature of 28.0 oC is found to occupy a volume of 20.3 liters. How many moles of Ar gas are in the sample?

Path A A sample of gas in a cylinder of volume 3.96 L at 327 K and 3.28 atm expands to 7.34 L by two different pathways. Path A is an isothermal, reversible expansion. Calculate the work for Path A. Answer in units of J. Path B Path B has two steps. In the first step, the gas.

A sample of gas at 38 degrees Celsius occupies a volume of 2.97 L and exerts a pressure of 3.14 atm. The gas is heated to 118 degrees Celsius and the volume decreased to 1.04 L. Determine the new pressure exerted by the gas.

A sample of gas collected over water at 42 C occupies a volume of one liter. The wet gas has a pressure of 0.986 atm. The gas is dried, and the dry gas occupies 1.04 L with a pressure of 1.00 atm at 90 C. Using this information, calculate the vapor pressure of water at 42 C.

a sample of gas occupies 500ml at STP. what volume will the gas occupy at 85.0 degrees Celsius

The volume of a sample of a gas collected over water at 32 Celsius and 752 torr is 627 ml. What will the volume of the gas be when dried and measured at STP? (Vapor pressure of water at 32 Celsius = 35.7 torr)

gont get it. To what temp must a sample of nitrogen at 27 degrees C and 0.625 atm be taken so that its pressure becomes 1.125 atm at constant volume i used the formula and it still gave me a weird answer

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.

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 atm pressure and 0.

A sealed container of volume 0.10 m3 holds a sample of 3.0 x 10^24 atoms of helium gas in equilibrium. The distribution of speeds of helium atoms shows a peak at 1100 ms-1. Caluculate the temperature and pressure of the helium gas. (helium atom 4.0 amu) How do I calculate the.

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 gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299K. If I raise the temperature to 350K and lower the pressure to 1.5 atm, what is the new volume of the gas? Use the combined gas law here. I will be happy to critique your work.

4. A container of gas has a volume of 3.5 L and a pressure of 0.8 atm. Assuming the temperature remains constant, what volume of gas would result if the pressure was 0.5 atm? A. 1.8 L B. 5.6 L C. 0.2 L D. 2.2 L My guess is B but I just want to double check

A sample of natural gas at STP is 78% CH4 and 22% C2H6 by volume how many moles of each gas are present in 1.60L of the mixture?

Hi I have 2 questions I hope someone can help me :) 1)A pocket of gas is discovered in a deep drilling operation. The gas has a temperature of 480c and is at a pressure of 12.8 atm. What volume of gas is required to provide 18.0 L of gas at the surface where the conditions are.

A cylinder of volume 2.3 L contains CO2 gas at 2.2 atm. A piston is pushed into the cylinder to decrease the volume to 1.2 L with no temperature change. What is the new pressure of the gas in atm? im completely stuck on how to start this.

1 ) A sample of vapor occupies a volume of 125 ml at 100 celcius and 748 torr. What is its volume under STP conditions? 2) A sample of vapor weighing 0.745 g filled a 250 ml flask when placed in a water bath at 98 degree celcius. The barometric presure that day was 753 torr.

a sample of gas has the pressure of 1120 mmhg and volume of 2.00 L. if the pressure is changed to 0.155 atm calculate the new volume

Suppose a 24.7 mL sample of helium gas at 25.°C and 1.14 atm is heated to 50°C and compressed to a volume of 14.8 mL. What will be the pressure of the sample? My teacher got 2.06 atm. pls explain to me how he got this. THANK YOU

a 500.0 mL gas sample at STP is compressed to a volume of 300.0 ml and the temperature is increased to 35.0 C. What is the new pressure of the gas in pascals?

What is the volume of 325 mL of a sample of gas at 51.0°C and 710. mm Hg if the conditions are adjusted to STP? Assume the amount of gas is held constant.

What is the volume of 325 mL of a sample of gas at 51.0°C and 710. mm Hg if the conditions are adjusted to STP? Assume the amount of gas is held constant.

Determine the atomic weight of X in the following compounds a)8g XH4 occupy 44.8L volume at 237C and 380 mmHg pressure b)1.92g of X3 occupis a volume of 574 ml at 77C and 2 atm c)A O.326 gram of gas,C3X4 has a volume of 250 ml at100C and 76 cmHg d)A 3.12 gram of the gaS.HX.

If 3.68 m^3 of a gas initially at STP is placed under a pressure of 3.61 atm, the temperature of the gas rises to 34.2 degrees C. What is the volume? Need step by step help.

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 108 atm 136 atm 219 atm

A sample of gas weighing 9.0 (g) at a pressure of 1 atm occupies a volume of 12.3 L. If the pressure is doubled,what is the resulting volume? (Assume constant temperature)

A spherical glass container of unknown volume contains helium gas at 25C and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25C, it is found to have a volume of 1.75 cm^3. The fas remaining in the first container shows a pressure of 1.710 atm.

A gas occupies a volume of 140 mL at 35 degrees celcius and 97 kPa. What is the volume of the gas at STP? Please show the work.

1. the molar mass of helium is 4.00 g/mol. calculate the volume of 1 mol of helium at STP (T = 273, P = 1 atm) what is the density of helium at STP? 2. the density

of an ideal gas is 1.35 kg/m^3. if the temperature is Kelvin and the pressure are both doubled, find teh new.

A 15.0L sample of argon has a pressure of 28.0 atm. What volume would this gas occupy at 9.90 atm? Assume ideal behavior.

A gas occupies a volume of 140 mL at 35 degrees celsius and 97 kPa. What is the volume of the gas at STP?

a gas has a volume of 410 mL at 27 degrees c and 740 mm Hg. what volume would this gas occupy at STP?

a gas has a volume of 410 mL at 27 degrees c and 740 mm Hg. what volume would this gas occupy at STP?

Initially 1.200 mol of an ideal gas in a container occupies a volume of 3.50 l at a pressure of 3.30 atm with an internal energy U1 = 547.2 J. The gas is cooled at a constant volume until its pressure is 1.80 atm. Then it is allowed to expand at constant pressure until its.

Initially 1.200 mol of an ideal gas in a container occupies a volume of 3.50 l at a pressure of 3.30 atm with an internal energy U1 = 547.2 J. The gas is cooled at a constant volume until its pressure is 1.80 atm. Then it is allowed to expand at constant pressure until its.

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.

A gas initially at STP is heated to 50°C keeping the volume constant. What is its new pressure? I used this formula: P1 = 1 atm T1 = 273 K T2 = 323 K solve for P2 P2 = P1 (T2/T1) But, where do I use the 50 degrees C? Also, is my answer correct: P2 = 1atm x 323K/273K = 1.18 atm

a gas volume has of v1=450ml. if the temp is held constant, what volume would gas occupy if the pressure p2=2p1? omg i cant figure anything out.

At 122C the pressure of a sample of nitrogen gas is 0.830 atm. what will the temperature in Celsius be at 3.00 atm, assuming constant volume.

what is the volume of a 2.00 gram sample of helium gas at STP?

A sample of gas in a balloon has an initial temperature of 28 and a volume of 1360. If the temperature changes to 86, and there is no change of pressure or amount of gas, what is the new volume. of the gas? Express the volume numerically in liters.

1. the molar mass of helium is 4.00 g/mol. calculate the volume of 1 mol of helium at STP (T = 273, P = 1 atm) what is the density of helium at STP? 2. the density of an ideal gas is 1.35 kg/m^3. if the temperature is Kelvin and the pressure are both doubled, find teh new.

Dr.Bob222: I attempted to solve the problem numerous times but keep ending up with the wrong answer. If you would be kind enough to show me the steps I would appreciate it. I'll pose the question once more: The volume of a gas at 24C and 0.21 atm is 36 mL. What volume will.

If the volume is 226 L at 1.7 atm, find the volume at 2.8 atm. Assume the temperature and amount of gas remain constant. Answer in units of L.

A 1.05 g sample of an ideal gas occupies 1.045 L at 20.0°C and 0.975 atm. What will be its volume at -8.6°C and 0.5 atm? I used PV=nRT for this. substituted P for 0.5 then n for 1.05, R .0821 then T for 264.4 K After doing this I got .0219 but it is incorrect, what am I doing.

An unknown gaseous hydrocarbon consists of 85.63% carbon by mass. A 0.335 g sample of the gas occupies a volume of 0.107 L at STP. What is the identity of the gas?

A volume of 2.0 L of He at 46 degrees celsius and 1.2 atm of pressure was added to a vessel that contained 4.5 L of N2 at STP. What is the total pressure and partial pressure of each gas at STP after the He is added?

A gas is compressed from an initial volume of 5.60 L to a final volume of 1.22 L by an external pressure of 1.00 atm. During the compression the gas releases 128 J of heat. What is the change in internal energy of the gas?

the highest pressure ever produced in a laboratory setting was about 2000000 atm. if we have a .000010 liter sample of a gas at that pressure until it is equal to 0.275 atm, what would the new volume of that gas be?

SHOW WORK A 44g sample of CO2 has a volume of 22.4 L at STP. The sample is heated to 71 degrees Celsius and compressed to a volume of 18.0 L. What is the resulting pressure?

A gas is at 31.3 atm pressure at 32 degrees C. The volume of the tank is 45.0L. What would the volume of the gas be if you allowed it to expand to a pressure of 55.3 atm?

IF A SAMPLE OF GASE HAVE A VOLUME OF 8.20 L AT 25*C AND 2.00 ATM, HOW MUCH VOLUME WILL IT TAKE UP IF YOU DECREASE THE PRESSURE TO 1.50 ATM AND INCREASE THE TEMPERATURE TO 100*C?

1.If the pressure of the gas in a 2.31 L balloon is 0.120 atm and the volume increases to 7.14 L, what will be the final pressure of the air within the balloon? Round to the nearest hundredth. Don't forget the units. 2.At a pressure of 2 atm, hydrogen gas occupies a volume of.

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

A gas at a pressure of 2.0 atm is contained in a closed container. Indicate the changes in its volume when the pressure undergoes the following changes at constant temperature. (Assume that the volume of the container changes with the volume of the gas.) The pressure increases.

1.If the pressure of the gas in a 2.31 L balloon is 0.120 atm and the volume increases to 7.14 L, what will be the final pressure of the air within the balloon? Round to the nearest hundredth. Don't forget the units. 2.At a pressure of 2 atm, hydrogen gas occupies a volume of.

A sample of O2 gas occupies 1.93L at a pressure of 10.0atm at 100 degree celsius. What volume will the sample occupy at stp?

The volume V of a gas varies inversely as the pressure P and directly as the temperature T. A certain gas has a volume of 20 L, and a temperature of 320 K, and a pressure of 1 atm. If the gas is compressed to a volume of 15 L and is heated to 330 K, what will the new pressure.

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 results if 60.0 mL of gas.

A 1.26 g sample of He gas has a pressure of 0.123 atm and a volume of 32.6 L. What is the temperature of the sample, in °C?

Use the molar volume of a gas at STP to calculate the density (in g/L ) of carbon dioxide gas at STP.

Initially a gas is at a pressure of 12 atm, a volume of 23 L, and a temperature of 200 K, and then the pressure is raised to 14 atm and the temperature to 300 K. What is the new volume of the gas? Round to the nearest tenth. Don't forget the units.

A sample of gas with a volume of 14.9 liters at 2.6 atmospheres pressure and a temperature of 25°C is allowed to expand to a volume of 29.3 liters at a temperature of 15°C. What is the final pressure (atm)atof the gas?

If a nitrogen gas sample occupies a volume of 2.55 L at 22.0 degrees Celsius and 0.860 atm, what is the mass of the N2 gas?

An ideal monatomic gas initially has a temperature of 333 K and a pressure of 7.15 atm. It is to expand from volume 581 cm3 to volume 1360 cm3. If the expansion is isothermal, what are (a) the final pressure (in atm) and (b) the work done by the gas? If, instead, the expansion.

Can you help me with this please - Temp - 650 Pressure - 690mm Hg mass - 0.927g volume - 194cm3 How do I calculate the volume of the gas at a different temp? & at a different pressure? You can do this two ways. The simplest is P1V2/T1 = P2V2/T2

If the student opened the bag after the above experiment, what would happen to volume of gas inside? A. The volume of gas in the bag will stay the same. B. the volume of gas in the bag will be decrease. C. The volume of gas in the bag will be increase. D. the volume of gas in.

1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas? 3. A 1.04-L sample of gas at 759 mm Hg pressure.

1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume? 2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas? 3. A 1.04-L sample of gas at 759 mm Hg pressure.

If I initially have a gas at a pressure of 13.5 atm, a volume of 2300 mL, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? Report the answer in correct number of significant figures.

Calcium metal and water produce hydrogen gas. If the volume of wet gas collected over water is 95.0 mL at 20 °C and 758 mm Hg, what is the volume of dry gas at STP conditions? (The vapor pressure of water at 20 °C is 17.5 mm Hg.)

If the pressure on a 2.50 mL gas sample were doubled from 0.500 atm to 1.00 atm, what would be gas volume at the new pressure? my Answer 1.25 mL if i'm wrong can you show me how u got to your answer please.

A balloon filled with 1.35 atm of dimethyl ether gas and 5.25 atm of oxygen gas at 27 °C has an initial volume 2.00L They react according to the following reaction: C2H6O (g) + 3 O2 (g) -> 2 CO2 (g) + 3 H2O (g) The system is allowed to back cool down to 27 °C following the.

(Ideal Gas Law) Calculate the volume of a 0.25 mole sample of gas at 25.0 degreeC and a pressure of 1.50 atm (R= 0.0821)

A helium balloon has a volume of 2.50L at STP. If it's released and rised to an elevation at which pressure is 0.285 atm, and the temperature is -35 degrees. What's the new volume?

A Sample of gas originally at 25 degrees C and 1 atm pressure in a 2.5 L container is allowed to expand until the pressure is .85 atm and the temperature is 15 degrees C. What is the final volume of gas? Did anyone get 2.6 L

A Sample of gas originally at 25 degrees C and 1 atm pressure in a 2.5 L container is allowed to expand until the pressure is .85 atm and the temperature is 15 degrees C. What is the final volume of gas? Did anyone get 2.6 L

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