Wednesday

April 16, 2014

April 16, 2014

Number of results: 51,428

**Chemistry**

The reaction for the decomposition of dinitrogen monoxide gas to form an oxygen radical is: N2O(g)==>N2(g)+O(g) . If the activation energy is 250 kJ/mol and the frequency factor is 8.0 x 1011 s-1, what is the rate constant for the first-order reaction at 1000 K? k = A * exp...
*Monday, March 1, 2010 at 8:12pm by gaby*

**chemistry help!!**

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) the answer is 1 mol ...
*Monday, March 21, 2011 at 12:54pm by Joanie*

**physics**

Three moles of an ideal gas are compressed from 5.5*10^-2 to 2.5*10^-2 m^3. During the compression, 6.1*10^3J of work is done on the gas, and heat is removed to keep the temperature of the gas constant at all times. Find the temperature of the gas. Can anyone please give me ...
*Sunday, March 2, 2008 at 2:40pm by Stella*

**PHYSICS**

Three moles of an ideal gas are compressed from 5.5*10^-2 to 2.5*10^-2 m^3. During the compression, 6.1*10^3J of work is done on the gas, and heat is removed to keep the temperature of the gas constant at all times. Find the temperature of the gas. Can anyone please give me ...
*Sunday, March 2, 2008 at 5:42pm by sTELLA*

**chemistry**

The solubility of nitrogen gas in water at 25 °C and 1 atm is 6.8!10"4 mol/L. If the partial pressure of nitrogen gas in air above water is 0.76 atm, what is the concentration of dissolved nitrogen?
*Monday, November 7, 2011 at 1:48pm by Anonymous*

**Chemistry**

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?
*Saturday, July 20, 2013 at 2:41pm by Sara*

**osu**

The ideal gas law states that for n moles of gas, the following relation applies: PV=nRT where P=pressure V=volume R=constant T=temperature in °K In the present case, P and n (and R) remain constant, from which we can conclude that the volume varies directly proportional ...
*Tuesday, November 23, 2010 at 12:02pm by MathMate*

**Physics**

The atoms in a gas (gas constant R=8.31 J/mol-K) can be treated as classical particles if their de Broglie wavelength ƒÉ is much smaller than the average separation between the particles d. Consider monatomic Helium gas (mHec2 = 3727MeV), molar mass 4g/mol) at 1.0 atmosphere ...
*Monday, December 7, 2009 at 6:40pm by Bun*

**Chemistry**

Consider the chemical reaction C + H2O -----> CO + H2 How many liters of hydrogen gas are formed From the complete reaction of 1.07 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and the temperature of 315K So I'm looking for volume and I have ...
*Wednesday, October 19, 2011 at 11:12pm by Monique *

**chem**

A sample of gas has an initial volume of 32.6L at a pressure of 1.2atm.If the sample is compressed to a volume of 13.4L , what will its pressure be? (Assume constant temperature.)
*Monday, October 7, 2013 at 4:11pm by kristine*

**CRC**

A sample of ideal gas is in a sealed container. The pressure of the gas is 675torr , and the temperature is 28\, ^{\circ}C . If the temperature changes to 91\, ^{\circ}C with no change in volume or amount of gas, what is the new pressure, P_2, of the gas inside the container?
*Sunday, April 28, 2013 at 2:42pm by Touch*

**algebra**

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...
*Tuesday, January 27, 2009 at 6:36pm by bob*

**chemistry**

Convert temperature to celsius. convert pressure to atmospheres. convert volume to liters. R=> gas constant. use PV=nRT P= pressure V= volume n= moles of gas R= gas constant T= temperature
*Tuesday, April 29, 2008 at 7:53pm by ~christina~*

**pressure**

4 mL of gas in a piston (syringe) at 10oC and 0.75 atm is heated and expanded to 85oC and 8 mL. What is the pressure of the gas after the expansion?
*Sunday, November 6, 2011 at 11:08pm by nja*

**Chemistry(Please check)**

1) Which statement below is incorrect if any? a)when gas is at STP, the pressure of the gas is at 1.00 atm. b)when a gas is at STP, the temperature of the gas is 25 degrees celsius c)at STP the molar volume of a gas is 22.4L d)at STP the molar volume of all gases are the same ...
*Wednesday, January 11, 2012 at 8:52pm by Hannah*

**chemistry**

A sample of gas is at a pressure of 1 atm , a volume of 1 L , and a temperature of 25 degrees celsius. What would happen to the pressure if the volume were reduced to 0.5 L and the temperature increased to 250 degrees celsius?
*Monday, November 8, 2010 at 11:12am by Anonymous*

**Chemistry**

A 108 mL gas sample has a mass of 77.96 mg at a pressure of 1140 mmHg and a temperature of 183 Â°C. Assume ideal gas behavior and a completely insulated system, and please donâ€™t forget units with your answers. The system is cooled. Calculate the amount of heat that will be ...
*Monday, March 10, 2014 at 11:30am by keitanako*

**Physical Chemistry**

Let's say we are given 1.0 mol of an ideal gas, and we are given a starting temperature, and and initial pressure the gas exerts. We are now told that the gas expands adiabatically until it reaches some other pressure, p2. How do we calculate w and dH for this? P, V, and T are...
*Wednesday, March 26, 2008 at 9:32pm by AJ*

**physics**

Start with part c). In case of an ideal gas, the internal energy only depends on temperature. In case of a monoatomic gas we have: E = 3/2 N k T here k is Boltzmann's constant and N is given as N = 7.1 mol = 4.276*10^24 So, we have: E = 88.55 J/K T If the temperature is raised...
*Wednesday, April 8, 2009 at 9:21pm by Count Iblis*

**chemistry**

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 1.00 *10^3 kg of water...
*Monday, March 8, 2010 at 1:54am by david*

**CHEMISTRY**

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.
*Monday, April 4, 2011 at 10:48pm by Anonymous*

**Physics**

A cylinder with a moveable piston holds 2.60 mol of argon at a constant temperature of 295 K. As the gas is compressed isothermally, its pressure increases from 101 kPa to 149 kPa. (a) Find the final volume of the gas. Answer in m3 (b) Find the work done by the gas. Answer in ...
*Friday, April 15, 2011 at 10:39am by steve*

**Chemistry**

A 10.8g sample of a gas has a volume of 5.25L at 25 degrees Celsius and 766mmHg. If 2.3g of the same gas is added to this constant 5.25L volume and the temperature raised to 68 degrees Celsius, what is the new gas pressure?
*Tuesday, January 18, 2011 at 7:09pm by Jen*

**chemistry**

PV = nRT P = 1 atmosphere V = 448 L (that sounds high, perhaps it is 4.48 L or sometime similar.) n = what you solve for. R = universal gas constant = 0.08206 L*atm/mol*K T = 273 K.
*Saturday, June 19, 2010 at 8:50pm by DrBob222*

**CHEM**

A GAS TAKES UP 25.2 L AT 25*C. AT 25*c THE GAS CAN ALSO TAKE UP 12.2lAT 1520 TORR. WHAT WAS THE PRESSURE IN ATM, OF THE ORIGINAL SAMPLE? I GOT 4.1S ATM. IS THAT RIGHT?
*Wednesday, August 1, 2012 at 7:17pm by liz*

**chemistry**

A 300 mL sample of hydrogen gas is at a pressure of 0.500 kPa. If the pressure increases to 0.750 kPa, what will be the final volume of the sample? Assume that the temperature stays constant
*Monday, February 13, 2012 at 9:08pm by Kristyn*

**chemistry**

A 300 mL sample of hydrogen gas is at a pressure of 0.500 kPa. If the pressure increases to 0.750 kPa, what will be the final volume of the sample? Assume that the temperature stays constant
*Monday, February 13, 2012 at 9:09pm by Kristyn*

**Chem Ideal Gas Law**

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 ...
*Thursday, November 1, 2012 at 6:58pm by Julie*

**chemistrty**

A sample containing 7.20g O2 gas has a volume of 33.0L Pressure and temperature remain constant. What is the volume after 4.00g He is added to the O2 gas already in the container?
*Friday, April 8, 2011 at 12:08am by nicole*

**physics**

A 22.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.40 105 Pa and temperature of 22.0°C. (a) Calculate the temperature of the gas in Kelvin. K (b) Use the ideal gas law to calculate the number of moles of gas in the tank. mol (c) Use the periodic table to compute ...
*Monday, April 29, 2013 at 11:01am by Annette*

**Chemistry**

Gas solubility increases: 1) Air in blood: a diver descends 10M, ad pressure increases by 1 atm. 2) The pressure of a gas over a solvent is increased. 3)The particle pressure of an anesthetic gas is increased. Gas solubility decreases: 1) O2: The temperature of a body of water...
*Wednesday, January 23, 2013 at 8:29pm by Anonymous*

**CHEMISTRY**

DETERMINE THE TEMPERATURE REQUIRED FOR 0.0354MOL OF GAS TO FILL A BALLOON TO 2.5L UNDER 0.998K PA PRESSURE PV = nRT. Change kPa to atmospheres and use R = 0.08206 L*atm/mol*K.
*Monday, January 8, 2007 at 10:19pm by TIFFANY*

**chemistry**

If 0.760 mol of solid TiO2 and 4.20 g of solid C are reacted stoichiometrically according to the balanced equation, how many liters of gaseous CO measured at STP are produced? 3TiO2(s) + 4C(s) + 6Cl2(g) ¡æ 3TiCl4(l) + 2CO2(g) + 2CO(g) Molar Mass (g/mol) TiO2 79.878 C 12.011 CO...
*Wednesday, June 2, 2010 at 6:16am by Judy*

**science: chemistry **

Use PV=nRT P is pressure in atm V is what you are looking for n is number of moles (1.5 mol) R is a constant( .08206) And T is temperature in Kelvin (22+273) PLUG AND CHUG
*Thursday, July 14, 2011 at 9:49am by CR*

**Physics**

A gas cylinder of volume 26 liters contains an ideal gas at temperature 27 degrees C and pressure 1920 kPa. Some of the gas leaks until the pressure falls to 1500 kPa. How many moles of gas leaked, assuming that the temperature remains constant during this process?
*Friday, January 17, 2014 at 5:37pm by Riley *

**chem**

How much water would be needed to completely dissolve 1.64 of the gas at a pressure of 750 torr and a temperature of 21 C? Henrys law constant is .145 M/atm.
*Sunday, September 12, 2010 at 10:52pm by moe*

**chem**

How much water would be needed to completely dissolve 1.64 L of the gas at a pressure of 750 torr and a temperature of 21 C? Henrys law constant is .145 M/atm.
*Monday, September 13, 2010 at 1:23am by moe*

**chemistry**

a gas sample is collected at 16 degrees c and 0.982 atm. if the sample has a mass of 7.40 g and a volume of 3.96 l, find the volume of the gas at stp and the molar mass?
*Tuesday, February 28, 2012 at 7:16pm by jessica*

**chemistry**

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.
*Saturday, January 19, 2013 at 1:10am by jakey *

**chemistry**

if PV=RT + ἁP where ἁ is a constant Calculate the work if the gas is heated at constant pressure from T1 to T2 Calculate the work if the gas is expanded isothermally and reversibly
*Wednesday, February 2, 2011 at 4:18pm by noel*

**physics**

ideal gas is kept under constant pressure of 1 atm. If initial temperature is 301K and the volume increases by 10% what is the final temperature of the gas? T2=? V1/V2= T1/T2 V1/V2= (301K)/T2 .10/1= (301K)/T2 Is the side with volume correct? The 10% part confuses me. Thanks ...
*Monday, December 3, 2007 at 6:42pm by Tammy*

**physics**

An ideal gas is kept under constant pressure of 1 atm. If initial temperature is 301K and the volume increases by 10% what is the final temperature of the gas? T2=? V1/V2= T1/T2 V1/V2= (301K)/T2 .10/1= (301K)/T2 Is the side with volume correct? The 10% part confuses me. Thanks...
*Monday, December 3, 2007 at 8:04pm by Tammy*

**Physics**

A 2.60-mol sample of oxygen gas is confined to a 5.03-L vessel at a pressure of 7.95 atm. Find the average translational kinetic energy of the oxygen molecules under these conditions.
*Saturday, June 22, 2013 at 12:20pm by Josie*

**Chemistry 140A**

A gas cylinder containing 6.38 mol of neon has a pressure of 491 mm Hg at 295 K. If 3.22 mol of helium is added to this cylinder, at constant temperature and volume, what will be the pressure in the cylinder?
*Tuesday, March 26, 2013 at 8:45pm by Ashley*

**Chemistry**

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.
*Sunday, May 13, 2012 at 8:37pm by Patrick*

**Chemistry**

An unknown amount of gas occupies 30.0 L at 2.1 ATM and 298K. How many moles does the sample contain? What is the mass if the gas is helium? What is the mass if the gas is argon?
*Wednesday, April 10, 2013 at 1:50am by Jake*

**Chemistry**

An unknown amount of gas occupies 30.0 L at 2.1 atm and 298K. How many moles does the sample contain? What is the mass if the gas is helium? What is the mass if the gas is argon?
*Wednesday, April 10, 2013 at 11:08pm by Ryan*

**Chemistry**

An unknown amount of gas occupies 30.0 L at 2.1 atm and 298K. How many moles does the sample contain? What is the mass if the gas is helium? What is the mass if the gas is argon?
*Friday, April 12, 2013 at 1:15am by Ryan*

**Chemistry**

Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.6 L of water upon warming from 25 C to 50 C. Assume that the water is initially saturated with nitrogen and oxygen gas at 25 C and a total ...
*Thursday, September 17, 2009 at 8:19pm by RE*

**Chemistry**

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?
*Monday, July 11, 2011 at 12:22am by Haley*

**physics**

So pressure will be 100 atm. Volume will be 3.10 L Temperature will be 296 K n will be 11 moles R will be 0.0821 (L*atm)/(mol*K) There is no unknown to solve for? I am confused..
*Thursday, November 19, 2009 at 2:58pm by sarah*

**Chemistry**

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 one decimal place, do...
*Monday, October 17, 2011 at 1:59pm by Javier*

**Chem**

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) __________________=.097mol NH3 .08201 x...
*Monday, October 5, 2009 at 4:10pm by Joe*

**Chemistry**

A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. How much volume will a 9.49 g sample of H2 occupy at 353 K and 2.00 atm? a. 68.2 L b. 54.7 L c. 147 L d. 109 L e.77.3 L Is it a. 68.2 L?
*Sunday, January 3, 2010 at 1:00am by Anonymous*

**Chemistry**

A sample of gas is placed in a container at 25 degrees C and 2 atm of pressure. If the temperature is raised to 50 degrees C, what is the new pressure?
*Thursday, February 17, 2011 at 11:27am by Cat*

**Chemistry**

A particular gas has a desnity of 11.98 g/dm^3 when the pressure is 138.4 kPa at a temp of 175 degrees F. What is the GMW of this gas? If it is a diatomic gas can you identify the element? dm^3 = L. so it's 11.98 g/L. then i converted 139.4 kPa to 1.37 atm. then i converted ...
*Thursday, September 6, 2007 at 6:57pm by Matt*

**Physics**

1.9 mol of gas at a temperature of -180 C fills a 3.4 L container. What is the gas pressure? Never been good at physics or mol stuff, how do you set it up?
*Friday, August 12, 2011 at 11:06pm by Catie*

**chemistry**

Phosphorus trichloride gas and chlorine gas reacts to form phosphorus pentachloride gas: PCL3(g) +CL2(g) = PCL5(g). A vessel is CHARGED WITH A MIXTURE OF PCL3(g) and CL2(g), which is allowed to equilibrate at 450K. At equlibrium the partial pressures of the three gases are ...
*Wednesday, October 19, 2011 at 3:23pm by MIndy*

**chemistry**

At a constant pressure, the volume of a gas is increased from 150.0 L to 300.0 L by heating it. If the original temperature of the gas was 20.0 degrees C, what will its final temperature (in Kelvin) be?
*Friday, February 24, 2012 at 11:14am by Dia*

**chemistry**

At a constant pressure, the volume of a gas is increased from 150.0 L to 300.0 L by heating it. If the original temperature of the gas was 20.0 degrees C, what will its final temperature (in Kelvin) be?
*Friday, February 24, 2012 at 11:14am by Dia*

**chemistry**

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.
*Monday, July 29, 2013 at 12:28am by rena*

**physics**

A chemist is working with a 4.50 mol sample of an ideal gas. The internal energy of the sample is known to be 14,900 J. What is the average kinetic energy of each gas molecule?
*Friday, March 14, 2014 at 12:21pm by Anonymous*

**10th Grade Honors Chemistry**

That is 3.97 moles of H2 gas. I assume that you know where that came from. I used 1.008 amu for the mass of an H atom. Each H2 molecule has two of them. Call 3.97 "n" and use the ideal gas law P V = n R T where T = 305 K You should look up and memorize the appropriate value of...
*Friday, March 26, 2010 at 1:42pm by drwls*

**OCHem**

The amount of methylcycloheane with the substituent in the equatorial orientation at room temperature (25C) would be The Gibbs free energy for axial methyl to equatorial methyl is -7.28Kj/mol (the universal gas constant is 8.314 j/deg-mol). I cant remember how to solve this...
*Friday, December 10, 2010 at 1:15pm by Alex*

**physical chemistry**

1.) Calculate delta rH for the freezing of water at one bar and -10 degrees C. The heat capacities are H2O(s)=36.9 JK-1mol-1 and H2O(l)=74.5JK-1mol-1. delta H for freezing of water at 0 degree C is -6602Jmol-1 (assume C is independent of temperature). 2.) Assume the hot brick ...
*Tuesday, February 21, 2012 at 5:03pm by nicole*

**chemistry**

the molar mass of an unknown gas was measured by an effusion experiment. it took 63s for te gas to effuse. where as nitrogen gas took 48sec. what is the molar mass of the gas? 32g/mol 37g/mol 24g/mol 16g/mol 48g/mol
*Monday, June 21, 2010 at 11:06am by Ellie*

**Chemistry**

The compound CH3F has van der Waals constants a = 5.009 atm•L2 /mol 2 and b = 0.0562 L/mol. Using both the ideal gas law and van der Waals’s equation, calculate the pressure expected for 25 mol of CH3F gas in a 5.00-L container at 75 °C. no idea how to even start this one...
*Saturday, December 1, 2012 at 11:54pm by Sarah*

**chemistry**

Hello, a few questions: Thanks so much! 1. The heat capacities of titanium and water are 0.522 J g-1 K-1 and 4.184 J g-1 K-1, respectively. What is the final temperature of the titanium-water mixture if a 175.0-g sample of titanium, initially at 90.0oC, is added to 50.0 g of ...
*Saturday, March 1, 2014 at 3:51pm by abby*

**chemistry**

Assuming the gas is ideal, we use Gay-Lussac's Law to relate the relationship between Temperature & Pressure of gas: P1/T1 = P2/T2 where: T1 = initial temperature of gas (in K) T2 = final temperature of gas (in K) P1 = initial pressure of gas P2 = final pressure of gas *note ...
*Wednesday, July 3, 2013 at 1:27am by Jai*

**chem**

a sample of gas is compressed from 3.25 l to 1.20 l at constant temperature. if the pressure of this gas in the 3.25 l volume is 100.00 kpa, what will the pressure be at 1.20 l ?
*Monday, April 5, 2010 at 7:59pm by hasan*

**PHYSICS**

A copper vat is 10 m long at room temperature (20 degrees C). How much longer it is when it contains boiling water at 1 atm pressure? Air in a balloon does 50 J of work while absorbing 70 J of heat. What is its change in internal energy? A bottle containing 3 kg of water at a ...
*Thursday, February 17, 2011 at 7:13pm by Matt*

**Chemistry**

A sample of zinc metal reacts completly with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) The hydrogen gas produced is collected over water at 25.0 °C. The volume of the gas is 78.0 L & the pressure is 0.980 atm. Calculate the amount of zinc metal ...
*Friday, August 12, 2011 at 7:51pm by ChemLover*

**chemistry**

A tank contains a mixture of 3.0 mol of nitrogen 2.0 mol of oxygen and 1 mol of carbon dioxide at 25 degrees and a total pressure of 10 ATM calculate the partial pressure in torr of each gas?
*Thursday, January 19, 2012 at 8:19pm by Lisa*

**chemistry**

A sample containing 4.8g of O2 gas has a volume of 15.0L. Pressure and temperature remain constant. What is the new volume if 0.500 mole of O2 gas is added?
*Friday, November 16, 2012 at 8:29pm by Boo Boo*

**chemistry**

A sample containing 4.8 g of O2 gas has a volume of 15.0L. Pressure and temperature remain constant. What is the volume after 4.00g of He is added to the 4.8g of O2 gas in the container
*Friday, November 16, 2012 at 8:55pm by Boo Boo*

**Chemistry**

Find the volume, in L, of 100g gas mixture containing 10.0 mol% hydrogen in nitrogen at 30.0C and 5.00 atm. Use the avg molecular wt. what is the molar concentration of hydrogen, in mol/L, in the gas mixture? what is the average mass denisity in g/L
*Thursday, July 26, 2012 at 4:19pm by Simon*

**Chemistry**

The volume of a sample of oxygen is 300.0mL when the pressure is 1.00 atm and the temperature is 27.0 degrees C. At what temperature is the volume 1.00 L and the pressure 0.500 atm?
*Tuesday, May 31, 2011 at 5:07pm by Kaitlin*

**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**

If 8.29 L of gaseous Cl2 measured at STP and 0.380 mol of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many moles of liquid CS2 remain? CS2(l) + 3Cl2(g) ¡æ CCl4(l) + S2Cl2(l) Molar Mass (g/mol) Cl2 70.906 CS2 76.143 CS2 1.26 Molar Volume (L...
*Wednesday, June 2, 2010 at 6:17am by Judy*

**Chemistry**

Suppose that 2.3 L of gas at 35°C and 1.0 atm is expanded to 4.5 L at 42°C. What will the final pressure of the gas be? (Ti in Kelvins=308.15; Tf(K)=315.15) Can someone please show me how to plug the values into the Combined Gas Law formula to calculate for Pf? Please don't ...
*Saturday, March 23, 2013 at 4:09pm by Pam*

**Eighth Grade Science**

A tube has gas within it whose volume equals 250 liters at a temperature of 300 celsius K . If the pressure of the gas is kept constant, what will the temperature be if the gas volume is increased by 50 liters ?
*Wednesday, November 19, 2008 at 5:06pm by Jordan*

**Chemistry**

350 calories of heat is added to a sample of nitrogen gas, and the temperature is increased by 89 degrees celsius. what is the mass of the sample of nitrogen gas? For this we'll presume that you are either given, or can find the specific heat of Nitrogen gas. Then plug them in...
*Tuesday, October 31, 2006 at 8:57pm by Allie*

**Chemistry**

An experiment shows a 144mL sample of gas has a mass of 0.173g at a pressure of 720mmHg at a temperature of 31 degrees celsius. what is the molar mass of the sample of gas?
*Monday, March 18, 2013 at 9:44pm by Sally*

**chemistry**

in the equation PV=nRT for gases what do each letter stands for? P is pressure (usually in atmospheres). V = volume in liters. n is number of mols R is the universial gas constant = 0.08206 liter*atm/mol*K T is termperature in Kelvin.
*Monday, January 29, 2007 at 8:43pm by claudia*

**engineering**

If the compartment is closed, the number of moles and volume are constant, so the ideal gas law tells you that P/T = constant where T is the absolute temperature. P2/T2 = P1/T1 P2 = (T2/T1)*P1 = 1273/293 = 4.345 atm
*Saturday, October 29, 2011 at 11:48pm by drwls*

**chemistry**

a gas occupies 37.6 L at 2.00 atm pressure and 27C degrees. how many moles of gas are present in this sample
*Wednesday, May 8, 2013 at 9:40pm by barbra*

**Chemistry**

A sample containing 4.80g of O2 gas has a volume of 15.0L. Pressure and temperature remain constant. What is the new volume if 0.500 mole of O2 gas is added? Am I converting the 4.80 O2 into moles first? How do I do that?
*Sunday, April 3, 2011 at 9:21pm by Shambrey*

**chemistry**

Start with the Ideal Gas Law PV = nRT or n = PV / RT K = n/P (from Henry's Law) n/P = V/RT (from the Ideal Gas Law) or K = V/RT (by combining the last two equations) (V = liters, R = 0.0821 L.atm/K.mol, T = 298K) Substitute to get the constant, K
*Thursday, September 17, 2009 at 8:28pm by GK*

**Chem**

Consider 1.40 mol of carbon monoxide and 3.20 mol of chlorine sealed in a 8.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) ↔ COCl2(g) Calculate the equilibrium molar concentration of CO. So I tried this question by finding the...
*Tuesday, February 12, 2013 at 5:13pm by Anonymous*

**chemistry**

Also this is assumed that it occurs at 1 atm. and the final temperature of the water is the same temperature of the gas.
*Thursday, November 5, 2009 at 5:37pm by Anmol*

**chemistry**

calculate the heat required to raise the temperature of 100g HCl gas from 300k to 800k at constant pressure Cp = 30j/k mol
*Tuesday, January 4, 2011 at 2:05pm by amira*

**chem 3A**

I am giving outlines below for solving problems #1 and #2. The others involve the same or similar principles. The general topic is reaction stoichiometry. It is hard to cover such a broad topic adequately through postings here. Question #1 (a) Use the Ideal Gas Law to find the...
*Friday, July 25, 2008 at 8:40pm by GK*

**Chemistry**

Given that KH for CO gas at 25 OC is 9.71 x10-4 mol.L-1.atm-1. Calculate the mass of CO that would dissolve in 1.00 L of H2O if the partial pressure of CO is 1.38 atm.
*Tuesday, February 15, 2011 at 12:17am by Chelsea*

**Chemistry**

A sample of hydrogen (2.02 g/mol) effuses through a porous container about 8.85 times faster than an unknown gas. Estimate the molar mass of the unknown gas. Answer in units of g/mol
*Tuesday, November 20, 2012 at 6:58pm by Caitlin*

**Chemistry**

A vessel of 9.49 L in volume contains 3.37 L of pure water at 25¡ÆC. A partial pressure of 4.73 atm of CO2 is quickly injected into the space above the water. Calculate the partial pressure of carbon dioxide remaining once the solution has become saturated with the gas. Henry'...
*Friday, February 2, 2007 at 2:36pm by Sally*

**Chemistry**

A vessel of 9.49 L in volume contains 3.37 L of pure water at 25¡ÆC. A partial pressure of 4.73 atm of CO2 is quickly injected into the space above the water. Calculate the partial pressure of carbon dioxide remaining once the solution has become saturated with the gas. Henry'...
*Friday, February 2, 2007 at 5:08pm by Sally*

**chemistry**

The gas phase reaction between nitrogen gas and oxygen gas to give NO gas is an endothermic process since 180.8 kJ of heat energy is absorbed when 1 mol of nitrogen reacts with 1 mol of oxygen. In which direction will the equilibrium be shifted if the temperature is increased...
*Wednesday, April 20, 2011 at 9:24pm by Rebekah*

**chemistry**

A 12 g sample of Ne is added to a container that also holds .78 mol of helium gas. What is the partial pressure of helium if the total pressure, after mixing is 2.43 atm?
*Friday, March 1, 2013 at 7:09pm by john*

**physics**

1.7 mol of an ideal gas which starts at 1.6 atm and 50 o C does 2.0 kJ of work during an adiabatic expansion. What is the final volume of the gas?
*Thursday, November 18, 2010 at 3:37pm by serena*

**chem/plz/check work studying for a final**

what is the volume occupied by 16.0g ethane gas (C2H6) at 720 Torr and 18C? V=nRT/P conversion of mol: 16.0g C2H6 X 1mol C2H6/30.07g C2H6= .53mol C2H6 V= .53 mol(0.0821 L*atm/mol*K)(291)K / 720 Torr (1 atm/760Torr) V= 13.5 L
*Thursday, December 16, 2010 at 10:15am by julia*

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