How many moles of chloroform, CHCl^3, are required to fill a 253-ml flask at 100.0 degrees Celsuis and 940 torr?

46,586 results

Chemistry

How many moles of chloroform, CHCl^3, are required to fill a 253-ml flask at 100.0 degrees Celsuis and 940 torr?

Chemistry

The vapor pressure of liquid chloroform, CHCl3, is 400.0 torr at 24.1 degrees Celsius and 100.0 torr at -6.3 degrees Celsius. What is delta Hvap of chloroform?

Chem

The vapor pressure of liquid chloroform, CHCl3, is 400.0 torr at 24.1°C and 100.0 torr at -6.3°C. What is ΔHvap (in the unit of kJ) of chloroform?

Chemistry

How many moles of a gas fill a flask with a volume of 141 mL at 101 degrees Celsius and a pressure of 761 torr?

Chemistry

What is the normal boiling point in ∘ C ^\circ {\rm C} of a solution prepared by dissolving 1.50 g {\rm g} of aspirin (acetylsalicylic acid, C 9 H 8 O 4 {\rm C}_{9}{\rm H}_{8}{\rm O}_{4}) in 75.00 g {\rm g} of chloroform (CHCl 3 ) ({\rm CHCl}_{3})? The normal boiling ...

Chemistry

The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...

Chemistry

How many moles of a gas at 100 degrees celciuos does it take to fill a 1.00 flask to a pressure of 1.50 atm?

Chemistry

The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...

Chemistry(Please help)

The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...

chemistry

A volatile liquid was allowed to evaporate in a 43.298g flask that has a total volume of 253 mL. The temp of the water bath wad 100 °C at the atmospheric pressure of 776 torr. The mass of the flask and condensed vaporous was 44.173g. Calculate the molar mass of the liquid

Chemistry

A compound has the empirical formula CHCL .A flask with volume 253 cm3 at temperature of 373K and pressure of 1.0 atm contains 0.8 g of the gaseous compound. Find the molecular formula of the compound.

Chemistry

A compound has the empiical fomula CHCl. a 256-mL flask, at 373 K and 750. Torr, contains 0.800 g of the gaseous compound. Give the molecular formula.

Chwmistry

how much in calories is required to raise the temperature of 415 grams of chloroform from 21.4 degrees c? The specific heat of chloroform is 0.23 cal/g°c. How many joules does this equal?

Chemistry

A compound has the empirical formula CHCl. A 256 mL flask, at 373 K and 750. torr, contains 0.800 g of the gaseous compound. Give the molecular formula.

Chemistry

The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...

chem

A 1.00 L flask containing 450 torr of H2 is connected to and mixed with a second flask with a volume of 0.500 L containing 250 torr N2. What is the final pressure of the resulting mixed gas system? a) 250 torr b)383 torr c) 450 torr d) 575 torr e) it cannot be determined

Chemistry

A flask was immersed in 350 g of water at 25 degrees C. Steam at 100 degrees C was passed into this flask, and eventually condensed into water at 100 degrees C. If the temperature of the water surrounding the flask was raised to 70 degrees C, how many grams of steam must have ...

Chem hw!

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 ...

Chem hw!

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 ...

Physics

a 500g piece of silver at 150 degrees celsuis is submerged in 1000g of water at 5 degrees celsuis to be cooled. determine the final temperature of the silver and water given. Cwater=4.18 x 10^3 J/kg.C Csilver = 2.4 x 10^2 J/kg.C

chemistry

determine the vapor pressure of a solution at 55 degrees C that contains 34.2g NaCl in 375 mL of water. The vapor pressure of pure water at 55 degrees C is 118.1 torr. so Psolution=XsolventPsolvent I don't know why I'm not getting the correct answer... so from 34.2g NaCl you ...

Chemistry

Consider three 1.0 L flasks at 25° C and 96.66 kPa containing the gases CH4 (flask A), CO2 (flask B), and C2H6 (flask C). In which flask is there 0.039 moles of gas? flask A flask C flask B none all

Chemistry

Consider three 1.0 L flasks at 25° C and 96.66 kPa containing the gases CH4 (flask A), CO2 (flask B), and C2H6 (flask C). In which flask is there 0.039 moles of gas? flask A flask C flask B none all

sciencee

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 ...

chemistry

Transfer the tablet to a clean 125-mL Erlenmeyer flask. Add 10-mL of 1M NaOH and heat the mixture to a gentle boil. Once the solution has cooled to room temperature, transfer it to a 100-mL vol. flask. Using the diluted solution from the 100-mL volumetric flask, rinse a 1-mL ...

chemistry

in a lab experiment to obtain the molar mass of a voltaile liquid, the following data is obtained: volume of flask=225ml mass of flask=77.834gms mass of flask+gas=78.416gms temperature=100 degrees celsius pressure=714 torr What is the molar mass of the liquid? A)11.1 g/mol B)...

chemistry

CoCl3(aq) + K2S(aq) yield Co2S3(s) + KCl(aq) How many moles of KCl would be produced when 0.470 moles of Co2S3 are produced in the above unbalanced reaction? How many moles of K2S would be required to react with 0.940 moles of CoCl3? How many moles of K2S would be required to ...

AP Chem

Would someone please check these for me? 52. In an experiment, you fill a heavy-walled 5.00-L flask with methane gas, CH4. If the flask contains 7.13 g of methane at 19 degrees C, what is the gas pressure? 2.14 atm 56. A 2.50-L flask was used to collect a 5.65-g sample of ...

chemistry

1 L FLASK CONTAINS NITROGEN ALONG WITH A DROP OR TWO OF WATER AT 40C THE TOTAL PRESSURE BEING 760 TORR .IF ALL THE CONTENTS ARE TRANSFERRED TO ANOTHER FLASK OF 0.5L AT THE SAME TEMPERATURE WHAT WILL BE THE PRESSURE SET UP IN THE SECOND FLASK? (AQUEOUS TENSION AT 40C = 55 TORR)

chemistry

1 L FLASK CONTAINS NITROGEN ALONG WITH A DROP OR TWO OF WATER AT 40C THE TOTAL PRESSURE BEING 760 TORR .IF ALL THE CONTENTS ARE TRANSFERRED TO ANOTHER FLASK OF 0.5L AT THE SAME TEMPERATURE WHAT WILL BE THE PRESSURE SET UP IN THE SECOND FLASK? (AQUEOUS TENSION AT 40C = 55 TORR)

chemistry

A flask that can withstand an internal pressure of 2511 torr, but no more, is filled with a gas at 21.0°C and 758 torr and heated. At what temperature will it burst? i used P1/x=P2/T2 and got 69.6 degrees Celsius. what is wrong

Chemistry

When dry and empty, a flask had a mass of 27.31 grams. When filled with distilled water at 25.0 deg C, it weighed 36.84 grams. After cleaning and drying, the flask was filled with chloroform and found to weigh 41.43 grams. At 25.0 deg C, the density of water is 0.9970 g/cm^3. ...

Dr. Bobb222

When you get a chance: If the pure liquid vapor pressure of benzene is 155 torr and the pure liquid vapor pressure of chloroform is 333 torr, then what is the total vapor pressure at 30°C of a solution of 9.26 g of benzene (C6H6) and 4.26 g of chloroform (CHCl3)? I get 195torr.

Chemistry

A 1.00 L flask is filled with Ar by water displacement at 20.0°C. the atmospheric pressure is 759.6 torr. after correcting for water vapor pressure in the flask, determine how many moles of Ar are present

Chemistry

Chloroform CHCl is an important solvent. It is produced by a reaction between methane and chlorine. How many g CH4 are needed to produce 50.0g CH4 +Cl3+ CH_4 + 3Cl_2 ->CHCl_3 + 3HCl}

science-chemistry

please anwser soon, a rigid 4.10L flask contains a mixture of 1.25 moles of H2, 0.250 mole of O2, and sufficient Ar so that the partial pressure of Ar in the flask is 1.00 atm. The temperature is 63.5 degrees C A) Calculate the total pressure in the flask B) calculate the mole...

CHemistry

My professor gave us these question in call and we solved for it in class, however im not sure how we got the answers. I dunt really understand the concept of intermolecular forces if some can please help me i have a quiz tomorrow. A. For each pair of substance, identify the ...

Chemistry

a. How many moles of N2 are present in a 1.00 qt flask that has a pressure of 425 torr at a temperature of 35°C? What is the mass in this na2? It would be much simpler to change quart to liters first, then torr to kpa PV=nRT n= PV/RT Temps in Kelvins, V in liters, P in kpa 1L...

organic chemistry

chloroform is an excellent solvent for extraction caffeine from water. Kd = 10 for caffeine in chloroform- water at 25 Celsius. what weight of caffeine would be removed from a solution of 4g caffeine in 100ml water by a single extraction of 100 ml of chloroform? for the ...

organic chemistry lab

chloroform is an excellent solvent for extraction caffeine from water. Kd = 10 for caffeine in chloroform- water at 25 Celsius. what weight of caffeine would be removed from a solution of 4g caffeine in 100ml water by a single extraction of 100 ml of chloroform? for the ...

OChem

The solubility of acetanilide is 3.53 g in 100 mL of chloroform at 0 °C, and 29.1 g in 100 mL of chloroform at 60 °C. What is the maximum percent recovery that can be achieved for the recrystallization of acetanilide from chloroform? Hint: During a recrystallization, some of...

Chemistry

a. How many moles of N2 are present in a 1.00 qt flask that has a pressure of 425 torr at a temperature of 35°C? What is the mass in this na2? It would be much simpler to change quart to liters first, then torr to kpa PV=nRT n= PV/RT Temps in Kelvins, V in liters, P in kpa I ...

Chemistry - Solubility

INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 M NaOH (7.5 mL of HCl needed to titrate) Flask C: 0.025 M NaOH (10.8 mL of HCl needed to titrate) Flask D: 0....

Chemistry - Solubility

INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: A 25 ml aliquot was used Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 M NaOH (7.5 mL of HCl needed to titrate) Flask C: 0.025 M NaOH (10.8 mL of HCl needed ...

Chemistry

a. How many moles of N2 are present in a 1.00 qt flask that has a pressure of 425 torr at a temperature of 35°C? What is the mass in this na2?

chemistry

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 ...

Chemistry

If the pressure of the gas inside the flask were increased and the height of the column in the open-ended arm went up by 0.5mm, what would be the new pressure of the gas in the flask, in torr? ANSWER IS 807.3 TORR

Chemistry

chloroform (chcl3) has a Hvap of 29.6 kj/mol and its boiling point occurs at 61.7c. the specific heat capacity of liquid chloroform is 0.622 J/gC while that of the gas is 0.714 J/gC. How much energy (in kJ) needs to be removed to condense 250 g of gaseous chloroform from 75.0C...

Chemistry

Two separate flasks are each filled with a gas at 25.0°C; the valve between them is opened and the gases are allowed to mix. What would be the final pressure in torr after mixing, if initially H2 is in the first flask (Volume = 4.000 L) at 271.8 torr and CCl4 is in the second...

Chemistry (Check)

6.3 mg of a boron hydride is contained in a flask of 385 mL at 25. degrees C and a pressure of 11 Torr. A. determine the molar mass of the hydride. B. which of the following hydrides is contained in the flask, BH3, B2H6, or B4H10 A. MM = 27.597 g/mol B. B2H6

chemistry

A 0.194 g sample of compound is vaporized to fill a 100.0 mL vessel at 750. torr and 100.C. What is the molar mass and molecular formula?

Chemistry

a 265 ml flask contains pure helium at a pressure of 756 torr. A second flask with a volume of 460 ml contains pure argon at a pressure of713 torr

Physics(Please check)

There is a rod that is split into two sections. The left side is copper with value of 390, temp of 100 degrees c and the length is 2m. The right side is silver, 420, temp 20 degrees celsuis, and length 1m. I need to calculate the temperature. 390 X 1 X 100-t / 2 = 420 X 1 X t-...

Physics(Please respond)

There is a rod that is split into two sections. The left side is copper with value of 390, temp of 100 degrees c and the length is 2m. The right side is silver, 420, temp 20 degrees celsuis, and length 1m. I need to calculate the temperature. 390 X 1 X 100-t / 2 = 420 X 1 X t-...

chemistry

a volatile liquid was allowed to evaporate in a 43.298g flask that has a total volume of 252 mL.,the temperature of the water bath was 100 celcius at the atmospheric pressure of 776 torr.the mass of the flask and condensed vapor was 44.173g.calculate the molar mass of the liquid.

chemistry

calculate the mass of chlorine gas contained in a 5dm3 flask at 25degrees celsuis and 98kpa pressure.

Chemistry PLEASE HELP!!

Procedure: 1. Calculate the mass of iron(II) ammonium sulfate hexahydrate, Fe(NH©þ)©ü(SO©þ)©ü*6H©üO (MW = 392.14) required to make 100 mL of solution that is 0.2M in Fe©÷⁺ ions. You will be asked to show your calculation in the Assignment. 2. Take a 100 mL ...

Chemistry

A vilatile liquid was allowed to evaporate in a 43.298 g flask that has a total volume of 252 ml. The temperature of the water bath was 100 degree Celsius at the atmospheric pressure of 776 torr. The mass of the flask and condensed vapor was 44.173 g. Calculate the molar mass ...

Chem1020

Consider the following balanced equation. 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table, showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as ...

chemistry

how many mole of air are there ina 125 mL flask if the pressure is 739 torr and the temperature is 18 degrees celsius?

Chemistry

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, ...

AP Chemistry

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 degrees Celsius of 1.0*10^-5 s^-1.Calculate the partial pressure of O2 produced from 1.00 Liter of 0.600 M N2O5 solution at 45 ...

chemistry

calculate the molar mass of an unknown whose mass was 0.846 g, and occupied a volume of 354 cm3 at a pressure of 752 torr and a temperature of 100 degrees celcius. I came up with .0114 moles, I want to know if this is correct.

AP CHEMISTRY

The molar mass of an unknown organic liquid (M~100) is determined by placing 5 mL of the liquid in a weighed 125-mL conical flask fitted with a piece of Al foil with a pin hole in it. The flask is heated in a boiling water bath until the liquid evaporates to expel the air and ...

Organic Chemistry

Assume that a round bottom flask holds 100 mL and the distilling head has an internal volume of 12 mL in the vertical section. At the end of a distillation, vapor would fill this volume, but it could not be forced through the system. No liquid would remain in the distillation ...

Chemistry

In an experiment, you fill a heavy walled 5.00 L flask with methane gas, CH4. If the flask contains 7.13g of methane at 19 degrees C, what is the gas pressure. Use the ideal gas law. Can some one help me get started on this problem please

chemistry

A volatile liquid was allowed to evorate in a 43.298g flask that has a total volume of 252mL.the temperature of the water bath was 100 celsius at the atmospheric pressure of 776 torr.the mask of the flask and condensed vapor was 44.173g.calculate the molar mass of the liquid. ...

Chemistry

Given PV=nRT and the following equation: CH4+2O2=CO2+2H2O Calculate the maximum number of ML of CO2 at 750 torr and 295.15 degrees K that can be formed from above conbution of methane ( CH4 ) if 450 mL of methane at 705 torr and 283.15 degrees K are mixed with 725 mL of O2 at ...

AP CHEMISTRY

The molar mass of an unknows organic liquid (M~100) is determined by placing 5 mL of the liquid in a weighed 125-mL conical flask fitted with a piece of Al foil with a pin hole in it. The flask is heated in a boiling water bath until the liquid evaporates to expel the air and ...

CHEM

The mass of an evacuated 255-mL flask is 143.187g. The mass of the flask filled with 267 torr of an unknown gas at 25 degrees Celsius is 143.289g. Calculate the molar mass of the unknown gas.

AP Chemistry

The answer is 50.0 torr and I got 46.0 torr but idk what I did wrong. Find the vapor pressure of a solution of 164 g of C3H8O3 and 338 mL of water at 39.8 degrees Celsius. Water's VP at 39.8 degrees celsius is 54.74 torr; it's density is 0.992 g/mL.

Chemistry Stoichiometry

The density of chloroform at a pressure of 220 mmHg and 25 degrees celsius is 1.42 g/L. Calculate the molar mass of chloroform. My set up is: mol*K .289 atm 1 1.42g/L ------------- ------------ ------ --------- .08206Latm 1 298K What I am unsure of is if this is the right way ...

CHEMISTRY 3

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, ...

chemistry

An equilibrium mixture of SO2,SO3 and O2 gases is maintained in a 11.5 L flask at a temp at which Kc=55.2 for the rxn shown below. If the number of moles of SO3 in the flask at equilibrium is twice the num of moles of SO2, how much O2 is present in the flask at equilibrium? ...

Chemistry

When 0.526 L of Ar at 1.20 atm and 227°C is mixed with 0.270 L of O2 at 501 torr and 127°C in a 400. mL flask at 27°C, what is the pressure in the flask?

Chemistry

When 0.578 L of Ar at 1.20 atm and 227°C is mixed with 0.299 L of O2 at 501 torr and 127°C in a 400. mL flask at 27°C, what is the pressure in the flask?

Chemistry

Preparing solutions a. A solution was prepared by dissolving 5.65 g potassium bromide in 32.67 g water. What is the concentration of this solution in weight percent? b. The solution was poured into a 100 mL volumetric flask and water was added to the mark on the flask. What is...

chemistry

A flask containing 5.00ml of 3M hcl solution required 14.45 of 1.00M naoh for titration. How many moles of hcl are present in the solution? The density of 3M hcl is 1.05g/ml. My calculation 0.005L x 3M = 0.015 moles 0.01445 x 1m = 0.01445 moles Who helps me to solve it

Chemistry

A sample of nitrogen gas is confined in a 8.494 L container at 2.643 x 102 torr and 50 oC. How many moles of gas are present in the sample? So I thought I set this problem up right and when I type the answer into CALM my answer is incorrect. This is what I did: PV=nRT (2.643 x...

Science

A sample of nitrogen gas is confined in a 8.494 L container at 2.643 x 102 torr and 50 oC. How many moles of gas are present in the sample? So I thought I set this problem up right and when I type the answer into CALM my answer is incorrect. This is what I did: PV=nRT (2.643 x...

Chemistry

A flask that can withstand an internal pressure of 2500 Torr, but no more, is filled with a gas at 21.0 C and 758 Torr and heated. At what temperature will it burst?

chemistry

A flask that can withstand an internal pressure of 2488 torr, but no more, is filled with a gas at 21.0°C and 758 torr and heated. At what temperature will it burst?

Chemistry

Could you help me with this question: A molecule of chloroform, CHCl3, has the same shape as a molecule of methane CH4. However, methane's boiling point is -164 degrees celcius ans chloroform's boiling point is 62 degrees celcius. Explain the difference between the two boiling...

Chem

0.600 L of Ar at 1.20atm and 227C is mixed with 0.200 L of O2 at 501 torr and 127 C in a 400ml flask at 27C. What is the pressure in the flask?

CHEMISTRY

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, ...

CHEMISTRY

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, ...

Chemistry

A 0.250-g sample of a magnesium-aluminum alloy dissolves completely in an excess of HCl (aq) . When the liberated H2 (g) is collected over water at 29 degrees celsius and 752 torr, the volume is found to be 301 mL . The vapor pressure of water at 29 degrees celsius is 30.0 ...

chemistry

I am trying to answer a bunch of lab questions about a lab I did and am stuck on finding the morality of the diluted vinegar solution? Can anyone help me? (I hope I gave enough info) Here where the lab procedures that I already went through: Transfer 10mls (Vc)of vinegar to a ...

Chemistry

Consider the following equilibrium at 1000K: 2SO2 (g) + O2 (g) ¡ê 2SO3 (g) A study of this system reveals that there are 3.5E-3 moles of sulfur dioxide gas, and 4.8E-3 moles of oxygen gas present in a 11.0L flask at equilibrium. The equilibrium constant for this reaction is ...

Chem

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, ...

MOLARITY QUESTION

I am trying to answer a bunch of lab questions about a lab I did and am stuck on finding the morality of the diluted vinegar solution? Can anyone help me? (I hope I gave enough info) Here where the lab procedures that I already went through: Transfer 10mls (Vc)of vinegar to a ...

chem

Nitrosyl Bromide Decomposes according to: 2NOBr(g) <=> 2NO(g) + Br2(g) *<=> is an equilibrium arrow( 1 mole each of NO and BR2 are in the flask. At equilibrium .60mol of BR2 remained. What is the number of moles of NOBr and NO in the flask at equilibrium, ...

chemistry

A 265- mL flask contains pure helium at a pressure of 747 torr. A second flask with a volume of 485 mL contains pure argon at a pressure of 721 torr .If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of helium?

Chemistry

An empty flask weighs 128.632g. After vaporization of a sample of volatile liquid, at a measured temperature of 99.8 C. The flask is sealed, cooled to room temperature, and weighed. The mass is now 129.225g. The measured P atm is 757.7 torr. The flask is rinsed and filled ...

Chemistry

An empty flask weighs 128.632g. After vaporization of a sample of volatile liquid, at a measured temperature of 99.8 C. The flask is sealed, cooled to room temperature, and weighed. The mass is now 129.225g. The measured P atm is 757.7 torr. The flask is rinsed and filled ...

Chemistry

The heat of combustion of bituminous coal is 2.5 x 10^4 J/g. What quantity of coal is required to produce the energy required to convert 100. Pounds of ice at 0.0 degrees Celsius to steam at 100.0 degrees Celsius?

Chemistry

The heat of combustion of bituminous coal is 2.5 x 10^4 J/g. What quantity of coal is required to produce the energy required to convert 100. Pounds of ice at 0.0 degrees Celsius to steam at 100.0 degrees Celsius? Is the answer 5.36 about right. I'm not sure if I did it correctly

Chemistry

a 3.67L flask is filled with carbon monoxide at 27 degrees C until the pressure is 1.27 atm. Calculate the total pressure after 3.42 moles of carbon dioxide has been added to the flask. (R=0.082 L-atm/K mol)

Chemistry

Cocaine is a non-electrolyte that has a molecular weight of 303.4 g/mole. How many grams must be dissolved in 25.0 mL of Chloroform (density = 1.484 g/mL) to raise its boiling point to 65.5 Celsius? The boiling point of pure Chloroform is 61.2 Celsius. Kb Chloroform = 3.62 ...

chemistry

2H2(g) + S2(g) ¡ê 2H2S(g) Analysis of the contents of a 15.0L flask reveals that there are 4.4 moles of hydrogen gas, 2.0 moles of sulfur gas, and 3.7 moles of hydrogen sulfide gas in the flask at equilibrium. Calculate the equilibrium constant K

Pages

  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15
  16. 16
  17. 17
  18. 18
  19. 19
  20. 20
  21. 21
  22. 22
  23. 23
  24. 24
  25. 25
  26. 26
  27. 27
  28. 28
  29. 29
  30. 30
  31. 31
  32. 32
  33. 33
  34. 34
  35. 35
  36. 36
  37. 37
  38. 38
  39. 39
  40. 40
  41. 41
  42. 42
  43. 43
  44. 44
  45. 45
  46. 46
  47. 47
  48. 48
  49. 49
  50. 50
  51. 51
  52. 52
  53. 53
  54. 54
  55. 55
  56. 56
  57. 57
  58. 58
  59. 59
  60. 60
  61. 61
  62. 62
  63. 63
  64. 64
  65. 65
  66. 66
  67. 67
  68. 68
  69. 69
  70. 70
  71. 71
  72. 72
  73. 73
  74. 74
  75. 75
  76. 76
  77. 77
  78. 78
  79. 79
  80. 80
  81. 81
  82. 82
  83. 83
  84. 84
  85. 85
  86. 86
  87. 87
  88. 88
  89. 89
  90. 90
  91. 91
  92. 92
  93. 93
  94. 94
  95. 95
  96. 96
  97. 97
  98. 98
  99. 99
  100. 100