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April 16, 2014

Search: barometric pressure of 765.7 mmHg is equivalent to 1.008 atm

Number of results: 14,213

Chemistry
Is barometric pressure of 765.7 mmHg is equivalent to 1.008 atm? I'm confused.
Wednesday, September 2, 2009 at 12:32am by Kedia

Chemistry
I'm trying to find the dry gas pressure of H2 in mmHg. The barometric pressure is 765.3 mmHg, the vp of H20 is 23.76 mmHg and the gas collected was 25.6 mL. this is what i did. 765.3 mmHg - 23.76 mmHg - (25.6 Ml/13.6 mmHg) = 739.66 = 740 mmHg 93 sig figs). Then I have to use ...
Wednesday, September 26, 2007 at 1:21pm by Clay

physics conversions
can you check my answers. 1. What is the corresponding barometric pressure values in mmHg if the barometric pressure is reported as: 29.7 inHg. = 754.38mmHg 31.8 inHg. = 807.72mmHg 26.4 inHg. = 670.56mmHg 22.1 inHg. = 561.34mmHg 34.8 inHg. = 883.92mmHg 2. What are the ...
Monday, January 28, 2008 at 4:21pm by james

physics conversions check my answers
can you check my answers. 1. What is the corresponding barometric pressure values in mmHg if the barometric pressure is reported as: 29.7 inHg. = 754.38mmHg 31.8 inHg. = 807.72mmHg 26.4 inHg. = 670.56mmHg 22.1 inHg. = 561.34mmHg 34.8 inHg. = 883.92mmHg 2. What are the ...
Monday, January 28, 2008 at 11:20pm by james

chemistry
A sample of O2 gas is collected over water at 23C at a barometric pressure of 751 mmHg (vapor pressure of water at 23C is 21 mmHg). The partial pressure of O2 gas in the sample collected is: (a) 21 mmHg (b) 751 mm Hg (c) 0.96 atm; or (d) 1.02 atm The answer is (c). Not sure ...
Wednesday, November 2, 2011 at 4:36pm by Holly

Chemistry
I have to chane the barometric pressure in my area to ATM. We have to look at the U.S. Weather map that gives the barometric pressure. I live in an area that has shows 1016 for barometric pressure. First is 1016 in millibars or what and secondly how do I convert that to atm so...
Tuesday, May 18, 2010 at 8:35pm by Hannah

chemistry
I figured it out. P total=751 mmHg. Partial pressure O2 + partial pressure H2O=751 mmHg. partial pressure O2=730 mmHg and 1atm/760 mmHg=x atm/730 mmHg. answer=0.96 atm! It was so easy I missed it....
Wednesday, November 2, 2011 at 4:36pm by Holly

Chemistry
A 70.8mL sample of "wet" O2(g) is collected over water at 29.9 degrees Celsius at a barometric pressure of 743 mmHg. The vapour pressure of water at 29.9 degrees Celsius is 31 mmHg. What is the mole fraction of O2 in the gas collected? So i found the partial pressure of O2 to ...
Saturday, October 16, 2010 at 5:10pm by Jon

Chemistry
A student reacts 0.1212 g of an Mg/NaCl mixture with hydrochloric acid. The volume of hydrogen saturated with water vapor collected at 20.0C was measured to be 42.7 ml. The column of water that remained in the buret was 10.3 cm high. If vapor pressure of water = 17.5 mmHg at ...
Wednesday, October 12, 2011 at 8:12pm by Duane

math
well, memorize this standard pressure is 101.3kPa 760 torr 760 mmHg 14.5 PSI 1 atm now, since all these are equal 2psi/14.5PSI=x mmHg/760mmHg solve for x mmHg then x mmWater= x mmHg* specificgravityHg now, convert xmmWater to inches x inch water= 25.4*xmmWhater
Saturday, December 11, 2010 at 8:15pm by bobpursley

Chem
Can someone check these homework answers please? 32. The barometric pressure measured outside an airplane at 9 km was 259 mmHg. Calculate the pressure in kPa. 34.5 kPa 36. A diving bell is a container open at the bottom. As the bell descends, the water level inside changes so ...
Tuesday, November 11, 2008 at 9:46pm by Anna

chemistry
Pressure of pure A at 85 (degrees)C is 500 mmHg, what is the vapor pressure of pure B at this temperature? A)336 mmHg B)960 mmHg C)576 mmHg
Sunday, June 27, 2010 at 6:58pm by jimbo

chem
the pressure 15 meters under water is 248 kPa what is the pressure in atm what is the pressure in mmHg
Tuesday, November 13, 2012 at 12:05am by christie

Chemistry
Data:O2 gas production Tria1 Trial 2 Mass of tube and contents prior to O2 production (g) 24.5196 g 24.4328 g Mass of tube and contents after O2 production (g) 24.4315 g 24.3513 g Mass of O2 generated (g) 0.0881 g 0.0815 g Moles of O2 generated (mol) 0.00275 mol 0.00255 mol ...
Wednesday, October 17, 2007 at 9:41pm by Taylor

Chemistry
I forgot in my previous question to say 1014 millibars. The question is I live at 1014 millibars for barometric pressure and temp. is 61 degrees Fahrenheit. I have an imaginary balloon that contains 22 grams of CO2-what is the volume in liters of the balloon using the gas ...
Wednesday, April 21, 2010 at 9:35pm by Robert

Chemistry
Data:O2 gas production Tria1 Trial 2 Mass of tube and contents prior to O2 production (g) 24.5196 g 24.4328 g Mass of tube and contents after O2 production (g) 24.4315 g 24.3513 g Mass of O2 generated (g) 0.0881 g 0.0815g Moles of O2 generated(mol) 0.00275 mol 0.00255 ...
Wednesday, October 17, 2007 at 9:41pm by Taylor

Bio 207
If barometric pressure is 480mmhg, what is the partial pressure of 02 in inspired air? At this pressure, what % of 02 would you have to gave in the air you are breathing so that the inspired p02 would be normal? ( 160 mmhg)
Monday, July 30, 2012 at 3:49pm by Sharon

chemistry
What is the effect of the following on the separation of the mixture? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate
Thursday, October 7, 2010 at 7:04pm by Anonymous

Physiology
If barometric pressure is 480mmhg, what is the partial pressure of 02 in inspired air? At this pressure, what % of 02 would you have to gave in the air you are breathing so that the inspired p02 would be normal? ( 160 mmhg)
Monday, July 30, 2012 at 12:54pm by Sharon

Chemistry
A mixture of hydrogen and oxygen gas has pressure of 1.60 atm. Partial pressure of oxygen is 304 mmHg atm, what is the partial pressure of hydrogen?
Tuesday, November 9, 2010 at 4:47pm by Sandra

Attn: DrBob222
A .326L container holds 0.146g of Ne and an unknown amount of Ar at 30C and the total pressure is 627 mmHg. Calculate the moles of Ar present? (I have calculated temp 308K, pressure is 0.825 atm and moles of Ne are .007) Chem - DrBob222, Wednesday, March 3, 2010 at 3:25pm T ...
Thursday, March 4, 2010 at 1:17pm by Staci

chemistry
What is the effect of the following on the separation of the mixture(hexane and toluene)? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate
Friday, October 8, 2010 at 8:32pm by Anonymous

chemistry
What is the effect of the following on the separation of the mixture(hexane and toluene)? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate
Saturday, October 9, 2010 at 10:53pm by Anonymous

chemistry
What is the effect of the following on the separation of the mixture(hexane and toluene)? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate
Thursday, October 14, 2010 at 2:57am by Anonymous

chemistry
What is the effect of the following on the separation of the mixture(hexane and toluene)? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate
Monday, November 8, 2010 at 5:33am by Anonymous

CHEMISTRY- vapour pressure
Bromobenzene, C6H5Br, and chlorobenzene, C6H5Cl, form essentially ideal solutions in all proportions. At 100C, the equilibrium vapour pressure of bromobenzene is 137mmHg and that of chlorobenzene is 285mmHg. Calculate the equilibrium vapour pressure above a 17.6% (w/w) ...
Saturday, October 9, 2010 at 7:38am by lulu

chemistry
What is the barometric pressure of water at 23.2 C, perferably in atm. Thank you.
Tuesday, January 19, 2010 at 6:35pm by anonymous

chemistry
express the barometric pressure in atm. 30.09Hg
Thursday, November 4, 2010 at 6:57pm by thomas richards

chem
The reaction AB(aq)->A(g)+ B(g)is second order in AB and has a rate constant of 0.0282 M^{-1} s^{-1} at 25 Celsius. A reaction vessel initially contains 250 mL of 0.105 M AB which is allowed to react to form the gaseous product. The product is collected over water at 25 ...
Friday, January 13, 2012 at 11:15pm by Yuni

Chemistry
Suppose a mixture of hydrogen and oxygen gas is exerting a pressure of 1.60 atm. If the partial pressure of oxygen in the mixture is 304 mmHg atm, what is the partial pressure of the hydrogen?
Friday, November 5, 2010 at 9:42pm by Amber

Chem
T is 303 and not 308 K which means you need to recalculate pressure and n for Ne. Use PV = nRT You can calculate moles Ne, plug that in for n, and plug in R, T, and V. Calculate pressure for Ne (I get something like 0.55 atm but I rounded here and there. That will be in atm so...
Wednesday, March 3, 2010 at 1:38pm by DrBob222

chem
A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25C, and the following equilibrium is achieved. N2O4(g)-> 2 NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.504 atm. (a) What is the equilibrium partial pressure of N2O4? for this...
Tuesday, February 19, 2013 at 4:55pm by Hannah

chem.
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
Tuesday, September 29, 2009 at 9:19am by Anonymous

chemistry
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?
Friday, April 2, 2010 at 10:27pm by fabiola

chemistry
What is the effect of the following on the separation of the mixture(hexane and toluene)? a. A soluble, nonvolatile impurity b. a decrease in barometric pressure c. an increase in barometric pressure d. rapid heating rate separation technique is distillation
Tuesday, November 9, 2010 at 7:41pm by Anonymous

chemistry
a tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?
Wednesday, November 14, 2012 at 8:33pm by Lauren

chemistry
The pressure in a constant-volume gas thermometer is 0.700 atm at 100C and 0.512 atm at 0C. (a) What is the temperature when the pressure is 0.0500 atm? C (b) What is the pressure at 405C? atm
Monday, April 29, 2013 at 10:55am by Anonymous

physics
a tank of ideal gas is sealed off at 20 degrees C and 1.00 atm pressure. What will be the pressure (in kPa and mmHg) in the tank if the gas temperature is decreased to -35degrees C ? the book answer is 82kPa = 6.2 x10^2 mmHg can you help me figure out how the book got this ...
Saturday, March 6, 2010 at 5:44pm by phyllis

chemistry
T = 765 K, PN2 = 31 atm, PH2 = 182 atm, PNH3 = 15 atm
Tuesday, May 1, 2012 at 7:21pm by Sarah

Chem
A sample of co2 gas at 90.7 degree celsius has a volume of 300. ml at 810 mmHg. How many moles of co2 are present R=.08206 L atm/mol K 1 atm=760 mmHg
Monday, December 3, 2012 at 4:14pm by hanah

Chemistry
A 2.50 L flask was used to collect a 5.65 g sample of propane gas, C3H8. After the sample was collected, the gas pressure was found to be 741 mmHg. What was the temperature of the propane in the flask. P= 741 mmHg(1 atm/760 mmHg)= .975 atm V= 2.50 L n= 5.65 g C3H8 (1 mol/44 g...
Tuesday, October 23, 2007 at 7:48pm by Lauren

Maths *have answer, want method* Urgent!
Suppose that the blood pressure of the human inhabitants of a certain Pacific island is distributed with mean, \mu = 108 mmHg and standard deviation , \sigma = 6 mmHg. According to Chebyshev's Theorem, at least what percentage of the islanders have blood pressure in the range ...
Saturday, April 13, 2013 at 12:40pm by Orla

Chemistry
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
Tuesday, November 29, 2011 at 5:50pm by erica

chem
Can someone glance over my work and see if it looks right? I'm certain about it because my units seem to be a little odd. Chloroform, CHCl3, has a vapor pressure of 197 mmHg at 23. degrees C and 448 mmHg at 45 degrees C. Estimate the heat of vaporization. ln P2/P1= heat of vap...
Friday, March 16, 2007 at 3:25pm by Chris

Chemistry
Convert all pressures to the same units, mmHg. Use the following relationships: 1 atm = 760 mmHg 1 torr = 1 mmHg 1 1 torr = 133.3 Pa
Sunday, June 14, 2009 at 10:04am by GK

physics
Tire pressure gauges do not read the absolute pressure, but the absolute pressure is what must be used when applying the ideal gas law. If the gauge says 2.2 atm, the actual absolute pressure is 3.2 atm. The absolute pressure at the higher temperature is then (323/298)*3.2 = 3...
Wednesday, May 26, 2010 at 1:43am by drwls

chemistry
We have a tank that contains O2 at 146 mmHg, N2 at 146 mmHg, and CO2 at 138 mmHg. We then add 135 mmHg of Ar. What is the pressure in the tank?
Sunday, May 5, 2013 at 4:31pm by Jenny

chemistry
We have a tank that contains O2 at 146 mmHg, N2 at 146 mmHg, and CO2 at 138 mmHg. We then add 135 mmHg of Ar. What is the pressure in the tank?
Monday, May 6, 2013 at 11:13am by Jenny

Chemistry
150.0 mL flask contains 740. g of N2 at 0C. 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 atm = 14.7 psi
Wednesday, February 26, 2014 at 4:37pm by Chelsey

Chemsitry
What is the phase of a compound at 600 mmHg and 32oC if it melts at 35oC when pressure is 760 mmHg? Its triple point occurs at 200 mmHg and 36oC.
Thursday, April 8, 2010 at 6:58pm by Dan

AP Chemistry
On a hot sunny day in August, the weather- man reports that the barometric pressure is 39 atm atmospheres. How many Pascals is this?
Sunday, October 13, 2013 at 11:36pm by Anonymous

Chemistry
5.0 dm^3= 5 Liters (P1V1/T1)=(P2V2/T2) P1= .92 atm V1= 5.0 L T1=? P2= (800 mmHg/760 mmHg)= 1.05 atm (There are 760 mmHg in 1 atmosphere) V2= 5.7 L T2= 30 degrees Celsius ((.92 atm)*(5.0 L))/(T1)=((1.05 atm)*(5.7 L))/(30 Degrees) 4.6/T1= .1995 4.16/.1995= T1 T1= 20.8 Degrees ...
Monday, November 19, 2012 at 7:28pm by Matt

AP Chem
Can someone please check these problems? 34. You fill a balloon with helium gas to a volume of 2.68 L at 23 degrees C and 789 mmHg. Now you release the balloon. What would be the volume of helium if its pressure changes to 632 mmHg but the temperature is unchanged? 3.35 L 38. ...
Wednesday, November 12, 2008 at 8:34pm by Anna

Chemistry
A sample of argon has a pressure of 1.021 atm at a temperature of 89.4 degC. Assuming that the volume is constant, at what temperature will the gas have a pressure of 1016.56 mmHg
Sunday, February 9, 2014 at 8:04pm by Anonymous

Chemistry
A sample of argon has a pressure of 1.021 atm at a temperature of 89.4 degC. Assuming that the volume is constant, at what temperature will the gas have a pressure of 1016.56 mmHg
Sunday, February 9, 2014 at 8:04pm by Anonymous

Chemistry
Any help would be great on the below problems. I am not sure where to begin. How do I solve these? Do I use a formula? 1. You are asked to make 500.0 mL of a 4.5M solution of HCl, but the only HCl you have available to dilute is 18.0M. Describe how you would make the desired ...
Tuesday, August 17, 2010 at 11:14pm by Ashley

chemistry
Water has an equilibrium vapor pressure of 23.8 mm Hg at 25 C. If 1.00 g H2O is sealed in a 20 L flask, what mass will remain in the liquid phase when equilibrium is established? ( 760 mmHg = 1 atm, R =0.0821 L.atm/mol.K)
Saturday, January 22, 2011 at 4:00pm by daniel

chemistry
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
Tuesday, May 4, 2010 at 8:25pm by Quentin

Chem
Please tell me if these are right? A mixture of oxygen and helium is prepared for a scuba diver that will descend to 125 feet below the ocean surface. At that depth the diver breathes a gas mixture that has a total pressure of 8atm. If the particle pressure of the oxygen in ...
Monday, November 29, 2010 at 1:29pm by Lindsay

chemistry
A mixture of CH4(g) at 0.500 atm and O2(g) at 0.750 atm is present in a 3.00-L container at 28C. 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 44C, after the reaction is complete? ...
Tuesday, October 3, 2006 at 6:43pm by geoff

Chemistry
If a sample of Helium gas is collected over water, what is the pressure of the dry gas alone if the total pressure is 760.0 mmHg and the partial pressure of water is 20.0 mmHg?
Sunday, January 10, 2010 at 6:57pm by Jane

Chemistry
A sample of oxygen is collected over water at a total pressure of 592.2 mmHg at 27C. The vapor pressure of water at 27C is 26.7 mmHg. What is the partial pressure of O2? ***Please show steps
Wednesday, March 7, 2012 at 9:43pm by Cindy

chemistry help me please
What values does STP have for pressure in the units of kPa and atm and mmHg?
Tuesday, June 1, 2010 at 5:22pm by Anonymous

Chemistry
yeah your off...180 mmHg is not the gas pressure. Instead, 180 mmHg is the difference between the gas pressure and the atmospheric pressure. i have the same problem...and i cant figure it out! your on the right track though!
Sunday, October 21, 2007 at 4:58pm by Major

Chem
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 pure water at this ...
Tuesday, March 27, 2007 at 8:32pm by Chris

Chemistry
A gas mixture with a total pressure of 750 mmHg contains each of the following gases at the indicated partial pressures: , 265 mmHg; Ar 134 mmHg; and ,O2 157 mmHg; The mixture also contains helium gas.
Tuesday, November 9, 2010 at 12:27am by Lisa

chem
if you mean 30C then here is the answer Air pressure = 763mmHg 298.7K ethanol pressure ? mmHG 303 K Total pressure of water= 980 mmHG 303 K you need to change air pressure to be based on 303 K after its been placed or immersed in water. P1/T1= P2/T2 (762 X 303)/ 298.7 = ? ? = ...
Sunday, April 26, 2009 at 6:51pm by ........

chem
The 3 atm (partial pressure) of H2 will combine with 1.5 atm (partial pressure) of O2 to produce 3 atm (partial pressure) of H2O, with 2.5 atm (partial pressure) of O2 left over. Thus 7 atm of reactants produces 5.5 atm of products + unreacted O2. I am assuming that the inital...
Friday, November 16, 2007 at 1:29pm by drwls

chemistry
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
Sunday, December 11, 2011 at 4:31pm by anonymous

Chemistry 105
A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO2, 257 mmHg; Ar, 123 mmHg; and O2, 160 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas...
Sunday, October 23, 2011 at 5:34pm by JULIE

Chemistry
A sample of iron reacted with hydrochloric acid. The liberated hydrogen occupied 40.1 mL when collected over water at 27 C at a barometric pressure of 750 torr. What is the mass of the sample of iron? (Because of the collection of gas over water, the vapor pressure of the ...
Monday, April 8, 2013 at 12:03pm by Kate

chemistry
ideal gas .450 mole initial pressure 16 atm and 290 K expands isothermally to a final pressure 1 atm. find work , if expansion is against a vacuum, a constant external pressure of 1 atm and reviersibly
Sunday, February 1, 2009 at 7:00pm by kat

chemistry
Just kidding. I'm stupid. I converted psi to mmHg and not atm to mmHg instead.
Wednesday, February 20, 2013 at 6:00pm by claire

Physics
pressure= atm pressure+ pressure pgh pressure due to height= pgh= 1000kg/m3 *9.8m/s* 11000m = 107800kPa 1atm=101.3Kpa so 107800kPa=1064.16 atm total pressure= 1+1064.16atm =1065 atm. =rounding to two sig fig: 1100atm
Thursday, November 12, 2009 at 9:00pm by miha

Chemistry
An open-ended mercury manometer is used to measure the pressure exerted by a trapped gas as shown in the figure. Atmospheric pressure is 750. mmHg. What is the pressure (in mmHg or torr) of the trapped gas if h =23 cm? I got 893.462, but that wasn't right. Can someone help ...
Wednesday, December 5, 2012 at 10:47am by Anonymous

ap chemistry
On a hot sunny day in August, the weather- man reports that the barometric pressure is 49 atm atmospheres. How many Pascals is this? Answer in units of Pascals
Saturday, February 9, 2013 at 7:08pm by cheri

chemistry
Calculate the pressure in atm of a balloon filled with 7.50g of helium gas if the balloon's volume decreases to 7.50L. Suppose the balloon's pressure and volume are originally 799 mmHg and 15.0L.
Tuesday, May 4, 2010 at 8:25pm by Quentin

ASAP help CHEMISTRY
A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?
Wednesday, December 19, 2012 at 10:09pm by Lisa

Chem
You measure two different pressures of the sealed vial containing air and ethanol at two different temperatures; 89027 mmHg at 27C and 90853 mmHg at 40C . From earlier measurements you found that the pressure of air at 27C is 76005 mmHg . Calculate the VPethanol at both ...
Monday, October 8, 2012 at 2:29pm by Anonymous

Chemistry
A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?
Saturday, October 30, 2010 at 4:01pm by Pat

PLEASE HELP-CHEMISTRY
A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr? ?
Wednesday, December 19, 2012 at 11:11pm by Will

Chem
A sample of co2 gas at 90.7 degree celsius has a volume of 300. ml at 810 mmHg. How many moles of co2 are present R=.08206 L atm/mol K 1 atm=760 mmHg is this correct? PV=nRT (1.07)(0.3)=(44.01)(.08206)(363.7) 0.3424=1313.49 =0.00026068 or 2.61^-4
Monday, December 3, 2012 at 4:47pm by hanah

chemistry
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
Monday, December 5, 2011 at 2:43pm by Anonymous

cleveland state university
A sample of gas at 1.3 atm of pressure is in a 2.0 L container. What will the pressure be if the sample is transferred to a 0.90 L container? 1. 0.59 atm 2. 1.4 atm 3. 2.9 atm 4. 3.2 atm
Monday, November 21, 2011 at 12:34pm by Danielle

chemistry
yes but the reason is the conversion factor is what I posted below Dr.Bob's comment to clarify on that. thus mmHg(760atm/mmHg)= atm
Tuesday, April 29, 2008 at 7:53pm by ~christina~

chemistry
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 equilibrium constant (Kp...
Thursday, April 8, 2010 at 12:14am by andy

chemistry
For A pressure of 25.7 inHg would be how many kilopascals? This is the answer I received: 25.7 mmHg x (101.325 kPa/760.0 mmHg) The mmHg cancel each other out So 98.659 kPa My Question is I started out with inHg, and not mmHg. Would it be the same since I'm starting with inHg? ...
Thursday, November 24, 2011 at 12:10pm by Sandy

CHEMISTRY
after starting with 0.343g Al and excess HCl the volume of H2 gas collected over water was 472ml. the atmospheric pressure was 754 mmHg and the temp was 21c. 1 balanced chemical equation? 2calculate the pressure in atm of dry hydrogen gas in a mixture
Thursday, April 18, 2013 at 6:39am by TJ

Chemistry
The dry gas pressure is pressure inside the tube - watervapor pressure. The pressure has nothing to do with the volume collected, unless you are supporting a column of water, then you have to adjust barometric pressure for the height of the column, it does not appear you had ...
Wednesday, September 26, 2007 at 1:21pm by bobpursley

chemistry
A sample of a saturated hydrocarbon is placed in a 1.0L vessel at 107oC. The pressure of the sample at these conditions is .40 atm. A stoichiometrically equivalent amount of oxygen is added to the vessel and the mixture is combusted. Following combustion, the pressure in the ...
Tuesday, May 22, 2012 at 6:42pm by bill

chemistry
A bearthing mixture used by deep-sea 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
Wednesday, March 16, 2011 at 5:19pm by Logan

chemistry
A gas mixture contains oxygen and argon at partial pressures of 0.60 atm and 425 mmhg. If nitrogen gas added to the sample increases the total pressure to 1250 torr, what is the partial pressure in torr?
Sunday, April 3, 2011 at 6:01pm by Jane

college chemistry
A sample of helium occupies 1521 mL at 719 mmHg. Assume that the temperature is held constant and determine a) the volume of the helium at mmHg. b)the pressure, in mmHg, if the volume is changed to 315mL
Tuesday, October 23, 2012 at 11:10pm by Haley

chemistry
ind the partial pressure of oxygen in a sealed vessel that has a total pressure of 2.6 atm and also contains carbon dioxide at 1.2 atm and helium at 0.10 atm.
Tuesday, May 4, 2010 at 3:11am by jerkoff

Chemistry
A weather balloon is inflated to a volume of 29.6 L at a pressure of 734 mmHg and a temperature of 27.0 C. The balloon rises in the atmosphere to an altitude, where the pressure is 360 mmHg and the temperature is -13.6 C.
Monday, November 8, 2010 at 11:26pm by Lisa

Math
7.5x102 = 765 let the amount of 11.98% mixture be x let the amount of 7.3% mixture be 765-x .1198x + .073(765-x) = .105(765) solve for x
Tuesday, November 22, 2011 at 10:28pm by Reiny

AP Chem
Next step is the combustion of gas B. The container is filled with gas B and oxygen to a combined total pressure of 11.98 atm (pressure gas B + pressure oxygen = 11.98 atm). The mixture is combusted, the pressure settles to 6.02 atm, MEANING that 11.98 atm - 6.02 atm = mols B...
Monday, January 21, 2008 at 12:06pm by DrBob222

physical chemistry
2 liters of N2 at 0 degree Celsius and 5 atm pressure are expanded isothermally against a constant pressure of 1 atm until the pressure of the gas is also 1 atm. Assuming the gas to be ideal, what are the values of work,delta E, delta H, and q for the process?
Saturday, September 29, 2012 at 11:10pm by lyn

Chemistry
You have 1L of an ideal gas at 0 degree celsius and 10 atm pressure. You allow the gas to expand against a constant external pressure of 1 atm, while the temperature remains constant. Assuming, 101.3 J/liter-atm, find q,w,delta E, and delta H in Joules, A) if the expansion ...
Friday, November 25, 2011 at 12:11pm by John

Chem
A .326L container holds 0.146g of Ne and an unknown amount of Ar at 30C and the total pressure is 627 mmHg. Calculate the moles of Ar present? (I have calculated temp 308K, pressure is 0.825 atm and moles of Ne are .007)
Wednesday, March 3, 2010 at 1:38pm by Staci

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