[rorygilmore1]

Any help is greatly appreciated.

Isooctane C8H18 undergoes combustion to form CO2 and H2O. How many moles of oxygen gas (O2) are needed to react completely with 1.25 moles of isooctane?


What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?

Also

A gas has a volume of 38.0ml at 23 degrees C and 97.8 atm of pressure. what will the volume be at standard temperature and pressure?

and

how many grams of water can be prepared when 2.00 moles of hydrogen and 2.00 moles of oxygen are mixed and reacted in this process? the formula is 2H2 + O2 -> 2 H2o

[sjb]

Any help is greatly appreciated.

Isooctane C₈H₁₈ undergoes combustion to form CO₂ and H₂O. How many moles of oxygen gas (O₂) are needed to react completely with 1.25 moles of isooctane?

So C₈H₁₈ + O₂  CO₂ + H₂O, does it? Can you balance this equation?

What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?

What concentration of hydrochloric acid are you using? Or alternatively, how many moles of HCl do you need?

A gas has a volume of 38.0ml at 23 degrees C and 97.8 atm of pressure. what will the volume be at standard temperature and pressure?

What is standard temperature and pressure?

how many grams of water can be prepared when 2.00 moles of hydrogen and 2.00 moles of oxygen are mixed and reacted in this process? the formula is 2H₂ + O₂ 2 H₂O

What does your balanced equation show you about the number of moles of hydrogen that react with oxygen, in relation to the amount of water produced?

[rorygilmore1]

Any help is greatly appreciated.

Isooctane C₈H₁₈ undergoes combustion to form CO₂ and H₂O. How many moles of oxygen gas (O₂) are needed to react completely with 1.25 moles of isooctane?

So C₈H₁₈ + O₂  CO₂ + H₂O, does it? Can you balance this equation?

Ok the balanced equation is  C₈H₁₈ + 9/2O₂ -> 8CO₂ + 9H₂O

What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?


What concentration of hydrochloric acid are you using? Or alternatively, how many moles of HCl do you need?

it is a 12.0 molar stock solution of hydrochloric acid

A gas has a volume of 38.0ml at 23 degrees C and 97.8 atm of pressure. what will the volume be at standard temperature and pressure?


What is standard temperature and pressure?

Standard temperature is 25 degrees Celsius which is 298K (25+273) Stard pressure is 1.00 atm

how many grams of water can be prepared when 2.00 moles of hydrogen and 2.00 moles of oxygen are mixed and reacted in this process? the formula is 2H₂ + O₂ 2 H₂O


What does your balanced equation show you about the number of moles of hydrogen that react with oxygen, in relation to the amount of water produced?

The coefficients of the Hydrogen and water are in a 2:1 ratio. The ratio of the hydrogen and the water are a 1:1 ratio. So could I set up a proportion with the grams of Hydrogen/2 (for the coefficient) = x grams/2?

[Think2Much4UserNames]

Any help is greatly appreciated.

Isooctane C8H18 undergoes combustion to form CO2 and H2O. How many moles of oxygen gas (O2) are needed to react completely with 1.25 moles of isooctane?


What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?

Also

A gas has a volume of 38.0ml at 23 degrees C and 97.8 atm of pressure. what will the volume be at standard temperature and pressure?

and

how many grams of water can be prepared when 2.00 moles of hydrogen and 2.00 moles of oxygen are mixed and reacted in this process? the formula is 2H2 + O2 -> 2 H2o

1. Balance equation first:
 

Then use stoichiometry.

2. What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?

    3.00M of what solution?

3. 
     Standard temperature: 25°C (298 K)
     . pressure: 1atm

[sjb]

Any help is greatly appreciated.

Isooctane C₈H₁₈ undergoes combustion to form CO₂ and H₂O. How many moles of oxygen gas (O₂) are needed to react completely with 1.25 moles of isooctane?

So C₈H₁₈ + O₂  CO₂ + H₂O, does it? Can you balance this equation?

Ok the balanced equation is  C₈H₁₈ + 9/2O₂ -> 8CO₂ + 9H₂O

So 1 mole of isooctane reacts with 4.5 moles of O₂, what about 1.25 moles?

What volume of hydrochloric acid (HCl) must be used to prepare 50.0ml of a 3.00M solution?


What concentration of hydrochloric acid are you using? Or alternatively, how many moles of HCl do you need?

it is a 12.0 molar stock solution of hydrochloric acid

How much HCl do you need in your new solution? What volume of 12.0 M HCl contains that number of moles?

A gas has a volume of 38.0ml at 23 degrees C and 97.8 atm of pressure. what will the volume be at standard temperature and pressure?


What is standard temperature and pressure?

Standard temperature is 25 degrees Celsius which is 298K (25+273) Stard pressure is 1.00 atm

OK, so how many moles of gas do you have initially?

how many grams of water can be prepared when 2.00 moles of hydrogen and 2.00 moles of oxygen are mixed and reacted in this process? the formula is 2H₂ + O₂ 2 H₂O


What does your balanced equation show you about the number of moles of hydrogen that react with oxygen, in relation to the amount of water produced?

The coefficients of the Hydrogen and water are in a 2:1 ratio. The ratio of the hydrogen and the water are a 1:1 ratio. So could I set up a proportion with the grams of Hydrogen/2 (for the coefficient) = x grams/2?

so 2 moles of hydrogen react with 1 mole of oxygen to give 2 moles of water? What's the mass of that?