Search: at a pressure of 1 atm

how many mm hg in 1 atm

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a mixture of 3 gases a, b and c is at a total pressure of 6.11 atm the partial pressure of gas a is 1.68 atm, that of gas b is 3.89 atm. what is the partial pressure of gas c?

A 355.0 mL cylinder containing SO3 at a pressure of 0.700 atm is connected by a valve to 0.559 L cylinder containing COCl2 at 380.0 torr pressure. Calculate the partial pressure (atm) of SO3 when the valve is opened. Unit conversion K = C + 273 1 atm = 760 torr Molar Mass (g/.

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 been rounded off to simplify.

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.

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?

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.

An ideal monatomic gas initially has a temperature of 338 K and a pressure of 6.96 atm. It is to expand from volume 435 cm3 to volume 1310 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.

An ideal monatomic gas initially has a temperature of 338 K and a pressure of 6.96 atm. It is to expand from volume 435 cm3 to volume 1310 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.

An ideal monatomic gas initially has a temperature of 338 K and a pressure of 6.96 atm. It is to expand from volume 435 cm3 to volume 1310 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.

suppose you were able to blow air out of your mouth at one third of an atmosphere pressure. How tall a column of water could your mouth air pressure push up a straw? I know atm pressure is 1 atm but I'm really confused about how to go about this problem. thanks!

Need help with #2 & # 3 1. Record the pairs of data for pressure (atm) and volume (mL). Pressure(atm) Volume(mL) 1.000 150 mL 1.154 130 mL 1.364 110 mL 1.667 90 mL 2. Does your experimental data verify Boyle's Law? Explain. 3. What pressure would the gas sample have at a.

an ideal gas in a closed inflexible container has a pressure of 6 atm and a temperature of 27 degree celsius. What will be the new pressure of the gas of temperature is decreased to -73 degree celsius? a) 2 atm b) 3 atm c) 4atm d) 8atm e) 9atm plz teach me the method also

an ideal gas in a closed inflexible container has a pressure of 6 atm and a temperature of 27 degree celsius. What will be the new pressure of the gas of temperature is decreased to -73 degree celsius? a) 2 atm b) 3 atm c) 4atm d) 8atm e) 9atm plz teach me the method also

The function p(d)=1+d/33, gives the pressure in atmospheres (atm), at the depth d in the sea (d is in feet). Note that p(0)=1 atm, p(33)=2 and so on. Find the pressure at 40 feet? I am lost please help? Thanks!

At 119 degrees C, the pressure of a sample of nitrogen is 1.94 atm. What will the pressure be at 282 degrees C, assuming constant volume? Answer in units of atm

if a gas is initially at 1.5 atm of pressure, Occupies a volume of 3.0 L at a tmepeature of 293K, what will be the new volume if the pressure increases to 2.5 atm and is now at 303K?

t 103 ◦ C, the pressure of a sample of nitrogen is 1. 89 atm. What will the pressure be at 275 ◦ C, assuming constant volume? Answer in units of atm

At 103◦C, the pressure of a sample of nitrogen is 1.89 atm. What will the pressure be at 275◦C, assuming constant volume? Answer in units of atm

A rigid tank contains 38:0 kg of O2 gas at a pressure of 9:70 atm. If the oxygen is replaced by helium, how many kilogram of helium will be needed to produce a pressure of 8:00 atm?

What will be the final volume of a 425 mL sample of gas initially at 22 degrees C and 1 atm pressure when the temperature is changed to 30 degrees C and the pressure to 0.471 atm?

A 12.8 L sample of Ne gas initially has a temperature of 32.7oC at a pressure of 2.57 atm. What is the new pressure, in atm, if the volume is changed to 10.6 L and the temperature is decreased to 13.9oC?

A mixture of He and O2 is placed in a 4.00L flask at 32 degrees Celsius. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4 atm. What is the mole fraction of O2. I don't understand how to do this.

A sample of methane gas at room temperature has a pressure of 1.50 atm and a volumne of 10.5 L. If the temperature is kept constant, what will be the new volume if the pressure is increased to 2.00 atm?

The initial pressure for the compounds involved in the reaction displayed were determined to be P(SO2(g)) = 0.5932 atm, P(O2(g)) = 0.4886 atm, P(SO3(g)) = 0.09287 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure of O2(g) was 0.

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

The function,p(d)=1+d/33, gives the pressure in atmospheres(atm), at a depth d in the sea (d is in feet).Note that p(0)=1 atm, p(33)=2, and so on. Find the pressure at 120 feet.

The function,p(d)=1+d/33, gives the pressure in atmospheres(atm), at a depth d in the sea (d is in feet).Note that p(0)=1 atm, p(33)=2, and so on. Find the pressure at 120 feet.

At what temperature does a 16.3 g of nitrogen gas have a pressure of 1.25 atm in a 25.0-L tank? Plz show me step by step how to do this, with using pressure as atm.

anonymous

A balloon is filled with 2.2 cm3 helium gas at 132.4 atm pressure. What will be the new pressure (atm) if the volume is changed to 68.6 cm3?

When a sample of neon with a volume of 683 mL and a pressure of 0.792 atm was heated from 19.0 to 76.0 °C, its volume became 733 mL. What was its final pressure (in atm)?

A pressurized can of whipping cream has an internal pressure of 1.035 atm at 28°C. If it is placed in a freezer at -15°C, what is the new value for its internal pressure?in atm

Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now calculate the work done if this process is carried.

The function p(d)=1+d/33, gives the pressure, in atmospheres (atm), at a depth d in the sea? (d in in feet). Note that p(0)=1 atm, p(33)=2, and so on. Find the pressure at 40 feet (Type answer as a integer or a simplified fraction.)

The function p(d)=1+d/33, gives the pressure, in atmospheres (atm), at a depth d in the sea (d is in feet). Note that p(0)=1 atm, p(32)=2 an so on. Find the pressure at 200 feet. Type an integer or simplified fraction.

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 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 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?

the function, p(d)=1+d/33, gives the pressure, in atmospheres (atm) at a depth in the sea (d is in feet). note that p(0)=1 atm, p(33)=2 and so on. find the pressure at 10 feet

Liquid helium at 4.2 K has a density of 0.147 g/mL. Suppose that a 1.00-L metal bottle that contains air at 118K and 1.0 atm pressure is sealed off. If we inject 120.0 mL of liquid helium and allow the entire system to warm to room temperature (25 °C), what is the pressure.

A 71.0 L cylinder containing CH2O at a pressure of 0.550 atm is connected by a valve to 1.50 L cylinder containing N2 at 266.0 torr pressure. Calculate the partial pressure (atm) of N2 when the valve is opened.

3 moles of an ideal gas initially at a pressure of 1 atm and a temprature of 100°C are expanded to twice the initial volume and then heated to 200°C at the new volume.What is the final pressure in atm?

A driving bell is a container open at the bottom. As the bell descends, the water level inside changes so that the pressure inside equals the pressure outside. Intially the volume of air is 8.58m^3 at 1.020 atm and 20 degrees C. What is the volume at 1.584 atm and 20 degrees C.

Each increase in pressure of 100 atm decreases the melting point of water by 1.0 degrees C. Estimate the temperature at which liquid water freezes under a pressure of 400 atm. How do I approach this problem?

Two moles of an ideal gas initially at 27C and 1 atm pressure are compressed isothermally and reversibly till the final pressure of the gas is 10 atm. Calculate the work done. (R=8.314 JK-1mol-1)

The pressure inside a hydrogen-filled container was 2.10 atm at 21 C. What would the pressure be if the container was heated to 86 C? Pfinal =. atm

A rigid container of O2 has a pressure of 3.5 atm at a temperature of 713 K. What temperature would be needed to achieve a pressure of 6.0 atm?

A balloon at contains 0.5 L of gas at a constant pressure of 1.0 atm. If the pressure is increased to 3.0 atm, what will be the volume of the gas?

A gas with a volume of 4.20 L at a pressure of 0.63 atm is allowed to expand until the volume raises to 95 L. What is the new pressure (in atm)?

A gas with a volume of 4.20 L at a pressure of 0.63 atm is allowed to expand until the volume raises to 95 L. What is the new pressure (in atm)?

A gas with a volume of 6.65 L at a pressure of 1.22 atm is allowed to expand until the volume raises to 54 L. What is the new pressure (in 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 fraction Ar = pAr/total p.

An office window has dimensions 3.6 m by 2.5 m. As a result of the passage of a storm, the outside air pressure drops to 0.925 atm, but inside the pressure is held at 1.0 atm. What net force pushes out on the window?

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?

An office window has dimensions 3.6 m by 1.6 m. As a result of the passage of a storm, the outside air pressure drops to 0.95 atm, but inside the pressure is held at 1.0 atm. What net force pushes out on the window?

A balloon at contains 0.5 L of gas at a constant pressure of 1.0 atm. If the pressure is increased to 3.0 atm, what will be the volume of the gas?

Need help with this question. Any help is appreciated. Heptane, C7H16, and octane, C8H18, form ideal solution. The solution boils at 85.00 єC and 0.522 atm. (At 85.00 єC, the vapor pressure of pure heptane is 0.570 atm and the vapor pressure of pure octane is 0.234 atm.) What.

A steel tank at 300 K contains 0.285 L of gas at 1.92 atm pressure. The tank is capable of withstanding a maximum pressure of 5.76 atm. Assuming that doubling the kelvin temperature causes the internal pressure to double, a. at what temperature will the tank burst? b. will it.

1 L of N_2_ gas, having a pressure of 2.5 atm, is added 1 L of Ar gas, having a pressure of 3.7 atm, in a sealed, rigid flask. What is the final pressure in the flask?

Calculate the partial pressures and total pressure (in atm) exerted by 0.838 mol of methane, 0.184 mol of ethane and 0.755 mol of neon contained in a 4.00 L container at 27 C. PV=nRT for methane (4.00L) X = (0.838 mol)(0.08206 L-atm/mol-K)(300.15 K) X = 5.160 atm PV=nRT for.

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?

A 10.0L flask contains 3.0atm of ethane and 8.0 atm of oxygen at 28 degrees C. The contents of the gas are reacted and allowed to return to 28 degrees C. What is the pressure of the flask? Using n=RT/PV I converted atm to moles and then used the balanced equation to find that.

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 3.00 atm. The partial pressure of hydrogen is 0.550 atm and the partial pressure of argon is 615 mm Hg. What is the partial pressure of helium?

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 2.90 atm. The partial pressure of hydrogen is 0.500 atm and the partial pressure of argon is 760. mm Hg. What is the partial pressure of helium?

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 2.55 atm. The partial pressure of hydrogen is 0.700 atm and the partial pressure of argon is 705 mm Hg. What is the partial pressure of helium?

Which of the following is NOT true about the thermodynamic standard state? A. A gas is in its standard state when its pressure is 1.00 atm and its temperature is 25C. B. An aqueous solution is in its standard state at a concentration of 1.00 M. C. A pure liquid is in its.

If helium added to the mixture increases the pressure to 1.90 <\rm atm>, what is the partial pressure (<\rm atm>) of the helium?

A cylinder with a moveable piston has a volume of 18.7 L at a pressure of 1.2 atm. What will be its volume if the pressure is increased to 1.7 atm?

A sample of gas at a pressure of 1.5 atm has a volume of 22.4 L. What is the new volume if the pressure is lowered to 0.75 atm?

A piece of solid carbon dioxide, with a mass of 6.2 g, is placed in a 4.0 L otherwise empty container at 21°C. ( a) What is the pressure in the container after all the carbon dioxide vaporizes? atm (.86 atm) (b) If 6.2 g solid carbon dioxide were placed in the same container.

A 69.4 L cylinder containing C2H6 at a pressure of 570 torr is connected by a valve to 105 L cylinder containing C6H6 at 0.350 atm pressure. Calculate the partial pressure (atm) of C6H6 when the valve is opened.

In an experiment, 238 mL of 0.45 molar hydrochloric acid completely reacts with excess iron to produce hydrogen gas and iron (III) chloride. What volume will the hydrogen gas occupy if it is collected over water at 35 degrees Celsius and 735 torr? The vapor pressure of water.

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temp of 112 degrees Celsius. What is the final volume of the gas, in milliliters, when the pressure and temp of the gas is changed to A.) 658 mmHg and 281K? B.) 0.55 atm and 75 degrees C C.)15. 4 atm.

Which of the following is NOT true about the thermodynamic standard state? A. A gas is in its standard state when its pressure is 1.00 atm and its temperature is 25C. B. An aqueous solution is in its standard state at a concentration of 1.00 M. C. A solid is in its standard.

Which of the following is NOT true about the thermodynamic standard state? A. A solid is in its standard state when the atmospheric pressure is 1.00 atm and the temperature is 25C. B. An aqueous solution is in its standard state at a concentration of 1.00 M. C. A gas is in.

Which of the following is NOT true about the thermodynamic standard state? A. A pure liquid is in its standard state at 25C and a vapor pressure of 1.00 atm. B. An aqueous solution is in its standard state at a concentration of 1.00 M. C. A gas is in its standard state when.

Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g)

A 150.0 mL cylinder containing CO at a pressure of 9.50 atm is connected by a valve to 9500 mL cylinder containing B5H9 at 2280 torr pressure. Calculate the partial pressure (atm) of B5H9 when the valve is opened.

A steel tank at 300 K contains 0.285 L of gas at 1.92 atm pressure. The tank is capable of withstanding a maximum pressure of 5.76 atm. Assuming that doubling the kelvin temperature causes the internal pressure to double, a. at what temperature will the tank burst? b. will it.

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) --> C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C

A container with a volume of 19.6 L that has temperature of 37C and a pressure of 0.900 atm has its temperature lowered to 0.00C and its pressure raised to 1.90 atm. What will the new volume be? Assume that the number of moles is constant.

A 2.9 L sample of gas has a pressure of 5 atm and a temperature of 50 °C. What will be the new temperature in Kelvin if the volume is decreased to 2.4 L and the pressure decreased to 3 atm? Round to the nearest whole number. Don't forget the units.

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

Calculate the value of the equilibrium constant (Kp) for the reaction shown, if F(g) was found to be 96.80 % decomposed at 1000 K when its initial pressure was 4.638 atm. The initial pressure of the reaction products is 0 atm. 2F(g) = F2(g)

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.

at 84 degrees Celsius. a gas in a container exerts a pressure of 0.503 ATM. assuming the size of the container remains the same, at what Celsius temperature would the pressure be 1.20 atm.

Air trapped in a cylinder fitted with a piston occupies 145.7 mL at 1.08 atm pressure. What is the new volume of air when the pressure is increased to 1.34 atm by applying force to the piston?

An aerosol can contains gases under a pressure of 4.6 atm at 18◦C. If the can is left on a hot sandy beach, the pressure of the gases increases to 4.69 atm. What is the Celsius temperature on the beach

A weather balloon carries instruments that measure temperature, pressure, and humidity as it rises through the atmosphere. Suppose such a balloon has a volume of 1.2 m^3 at sea level where the pressure is 1 atm and the temperature is 20°C. When the balloon is at an altitude of.

If the initial pressure of HD(g) is 2.270 atm, calculate the % decomposition of HD(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 727.0 °C is 0.26. The initial pressure of the reaction products is 0 atm. 2HD(g) = H2(g)+D2(g)

Before beginning a long trip on a hot day, a driver inflates an automobile tire to a gauge pressure of 2.20 atm at 300 K. At the end of the trip, the gauge pressure has increased to 2.70 atm.

A 3.43 L flask is filled with carbon monoxide at 27 °C until the pressure is 8.31 atm. Calculate the total pressure after 2.09 moles of carbon dioxide has been added to the flask. (R=0.082 L-atm/K mol)

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?

Exactly 1.0 mole of oxygen and 7.0 moles of nitrogen gas are in a container. The total gas pressure is 5.7 atm. What is the partial pressure of nitrogen in atm? I'm not sure how to go about setting up the problem. Any help is appreciated!

a tank contains 26.0 kg of oxygen gas at a gauge pressure of 8.70 atm. if oxygen is replaced by helium, how many kilograms of the latter will be needed to produce a gauge pressure at 7.00 atm?

In an experiment, 25.0 ml of a gas with a pressure of 1. atm is contained in a balloon at 25.0 c. The Balloon is then cooled to 5.0 c, and the pressure is found to be .750 atm. What is the volume of the gas under the new conditions?

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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