Chemistry, 13.12.2019 21:31 haileyhale5

The large bulb, with a volume of 6.00 l, contains nitric oxide at a pressure of 0.500 atm, and the small bulb, with a volume of 1.50 l, contains oxygen at a pressure of 2.50 atm. the temperature at the beginning and the end of the experiment is 22 °c. what are the partial gasses of no, and no2?

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Answer from: girlhooper4life11

P(O2) = 0.300 atm

P(NO2) = 0.400 atm

P(NO) = 0 atm

Explanation:

Step 1: Data given

Volume of large bulb = 6.00L

Large bulb contains nitric oxide at 0.500 atm

Volume of the small bulb = 1.50 L

Small bulb contains oxygen at 2/50 atm

The initial temperature = 22.0°C

Step 2: The balanced equation

2 NO + O2 → 2 NO2

Step 3: Calculate moles of NO

P*V=n*R*T

n = (P*V)/(R*T)

⇒ with P = the pressure of NO = 0.500 atm

⇒ with V = the volume of NO = 6.00L

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 22.0 °C = 295 K

⇒ with n = the number of moles of NO

n(NO) = (0.500 *6.00)/(0.08206*295)

n(NO) = 0.124 moles

Step 4: Calculate moles of O2

n = (P*V)/(R*T)

⇒ with P = the pressure of O2 = 2.50 atm

⇒ with V = the volume of 02 = 1.50 L

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 22.0 °C = 295 K

⇒ with n = the number of moles of O2

n(O2) = (2.50*1.50)/(0.08206*295)

n(O2) = 0.155 moles

Step 5: Calculate the limiting reactant

For 2 moles NO consumed, we need 1 mole O2 to produce 2 moles of NO2

No is the limiting reactant. It will completely be consumed. (0.124 moles)

O2 is in excess. There will react 0.124/2 = 0.062 moles O2

There will remain 0.155 - 0.062 = 0.093 moles O2

Step 6: Calculate moles of NO2

For 2 moles NO consumed, we need 1 mole O2 to produce 2 moles of NO2

For 0.124 moles NO, we'll have 0.124 moles NO2

Step 7: Calculate partial pressure of O2

P*V= n*R*T

P = (n*R*T) / V

⇒ n = the number of moles O2 = 0.093 moles O2 remain

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature = 295 Kelvin

⇒ V = the volume = 6.00 + 1.50 = 7.50 L

P(O2) = 0.300 atm

Step 8: Calculate partial pressure of NO2

P = (n*R*T) / V

⇒ n = the number of moles NO2 = 0.124 moles

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature = 295 Kelvin

⇒ V = the volume = 6.00 + 1.50 = 7.50 L

P(NO2) = 0.400 atm

P(NO) = 0 atm because NO is completely consumed.

Answer from: Quest

Since there is the same amount of agn03 in both silver chloride and silver nitrate they produce the same amount of moles. therefore silver chloride produces the same amount of silver nitrate, so your answer is 15.0 moles of silver nitrate. i hope this !

Answer from: Quest

Mass is the amount of matter in an object. weight is the measurement of the pull of gravity on an object. say for example, you travel to the moon which has a different gravitational field compared to the gravitational field of earth. (gravitational fields: earth = 1, moon = 0.165) now when you are on the moon, the pull of gravity on you is different than on the earth. and as weight is the measurement of the pull of gravity on an object, that means yes, your weight can and will change on the moon. however, on the moon, on earth or even on jupiter, the amount of mass inside of you remains the same. meaning your physical mass remains constant. in conclusion it is possible for your weight to change as your mass remains constant.

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