
How many litters of Oxygen will be required to burn 3.8 liters of propane, C3H8?

What volume of oxygen gas at 20.9 c and 750 torr is needed to burn 3.00 liters of propane, C3H8 at the same temprrature and pressure? I know i use V1/n1=V2/n2, but how do i get n?

In the following reaction, how many liters of oxygen will react with 124.5 liters of propane (C3H8), at STP? C3H8 + 5O2 = 3CO2 + 4H2O

what mass of oxygen would be required to completely burn 6.75 g of propane in the following reaction? C3H8+5O2 => 3CO2+4H2O * please help

Consider the combustion of propane (C3H8) in the presence of oxygen: C3H8+5O2 => 3CO2+4H2O How many grams of O2 are required to react completely with 3 moles of propane?


Consider the combustion of propane (C3H8) in the presence of oxygen: C3H8+5O2 => 3CO2+4H2O How many grams of O2 are required to react completely with 3 moles of propane?

Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O). Write a balanced equation for this reaction. Assuming that all volume measurements occur at the same temperature and pressure,

Propane gas (C3H8) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide gas (CO2) and water vapor (H2O). Write a balanced equation for this reaction. Assuming that all volume measurements occur at the same temperature and pressure,

C3H8 + 5O2 3CO2 + 4H2O How many grams of oxygen are required to burn 7.0 g of C3H8?

consider C3H8+O2=CO2+H20 how much oxygen would be needed to completely burn 250g of propane

Complete combustion of propane (C3H8). How many grams of water are produced when 50 grams of propane are reacted with 101 liters of oxygen @STP? Please explain in deminsionsl analysis and how you type it in the calculator. Thanks c:

How many grams of oxygen are required to react with 2.50 g of propane (C3H8) to form CARBON MONOXIDE and water? this is what i did why is it wrong? 2.50 g C3H8 x 1 mole / 44.09 g C3H8 x 5mole O2 / mole = 9.1 g O2 everything cancels to get grams of O2 which

propane(C^3H^8)is used as a fuel. Propane is a type of hydrocarbon. Write a balanced equation for the combustion of propane in oxygen. Assume that the combustion is complete. Hydrocarbons (C and H compounds of which propane is one) burn in oxygen to

Could someone please walk me through step by step on how to do this. Propane (C3H8) burns in oxygen to produce carbon dioxide and water. C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 48.2 g propane

Many home barbecues are fueled with propane gas (C3H8). How much carbon dioxide in kilograms is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5gal tank)? Assume that the density of the liquid propane in the tank


A small bottle of propane gas (C3H8) contains 400.0 grams of propane. When the propane is burned in oxygen, how many moles of each product are formed?

In a combustion reaction, propane (C3H8) reacts with oxygen. How many moles of CO2 can be produced when 2.25 mol of C3H8 react? C3H8(g) + 5O2(g) „³ƒn3CO2(g) + 4H2O(g)

For the following reaction, 5.20 grams of propane (C3H8) are allowed to react with with 23.1 grams of oxygen gas. propane (C3H8) (g) + oxygen (g) carbon dioxide (g) + water (g) What is the maximum amount of carbon dioxide that can be formed? grams What is

Propane (C3H8) is burned in oxygen to pro duce carbon dioxide and water. The heat of combustion of propane is 2012 kJ/mole. How much heat is given off when 3.0 mol C3H8 are reacted with 10.0 mol O2?

propane (c3h8) is burned in oxygen to produce carbon dioxide and water. The heat of combustion of propane is 2012 kJ/mole. How much heat is given off when 3.0 mol C3H8 are react with 10.0 mol O2? Thanks, and please if possible show all steps!

StoichiometryI have the basic strategy, but am still stuck on how to do them.example...propane burns in oxygen according to the following reaction C3H8 + O2 produces CO2 + H20 a. How many moles of CO2 are formed when 2.8 g of propane reacts? b. If 0.45 g

When using a limited quantity of oxygen to react with propane (C3H8), this will result in producing carbon monoxide (CO) and carbon dioxide (CO2) gases. If 25% of 128 g of propane used in such process is converted into CO and the rest into CO2, calculate:

Given this equation. C3H8 + 5O2 > CO2 + H2O. How many moles of O2 will be needed to comepletely burn 1.75 moles of propane C3H8?

Propane, C3H8, reacts with oxygen according to the following balance equation. If 44 grams of propane react completely with sufficient oxygen, how many grams of water are produced?

The combustion of propane is given by the following reaction: C3H8 (g) + 5 O2 (g) > 3 CO2 (g) + 4 H2O (g) If 5.00 L of propane are burned in in the presence of excess O2, how many liters of carbon dioxide will be formed?


Propane(C3H8), the major component of LP game, is often used as heating and cooking fuels in homes. When propane is burned( reacted with oxygen), CO2(g) and H2O(g) are produced. 1) Write an equation for the reaction and calculate the enthalpy change for

What mass of propane (C3H8) is needed to produce 346 g carbon dioxide in the following reaction? C3H8(g) + 5O2(g) > 3CO2(g) + 4H2O(g) A. 346 g C3H8 B. 115 g C3H8 C. 5075 g C3H8 D. 1.86 g C3H8

What mass of propane (C3H8) is needed to produce 346g carbon dioxide in the following reaction? C3H8(g)+5O2(g)> 3CO2(g) +4H2O(g) A. 115g C3H8 B. 1.86g C3H8 C. 5075g C3H8 D. 346g C3H8

Propane (C3H8) is burned in oxygen to pro duce carbon dioxide and water. The heat of combustion of propane is 2012 kJ/mole. How much heat is given off when 3.0 mol C3H8 are reacted with 10.0 mol O2? 1. 4024 kJ 2. 2012 kJ 3. 916 kJ 4. 1555 kJ 5. 5122 kJ

In the complete combustion of C3H8 (propane), how many liters of CO2 are produced from 10 liters of O2?

If 120. g of propane, C3H8, is burned in excess oxygen according to the following equation: C3H8 + 5O2 3CO2 + 4H2O, how many grams of water are formed?

How many liters of oxygen are required to react completely with 5.9 L c3H8?

Oops I posted the right question but wrong answer options... What mass of propane (C3H8) is needed to produce 346g carbon dioxide in the following reaction? C3H8(g)+5O2(g)>3CO2(g)+4H2O(g) A. 346g C3H8 B. 115g C3H8 C. 5075g C3H8 D. 1.86g C3H8

Consider the combustion of propane: C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l) delta H= 2221 kJ Assume that all of the heat comes from the combustion of propane. Calculate delta H in which 5.00g of propane is burned in excess oxygen at constant pressure.

Consider the combustion of propane: C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l) delta H= 2221 kJ Assume that all of the heat comes from the combustion of propane. Calculate delta H in which 5.00g of propane is burned in excess oxygen at constant pressure.


The combustion of 132 g of propane, C3H8, with excess oxygen liberates 6.6x10^3 kj of heat. What is the enthalpy change for the reaction below: C3H8(g) + 5O2(g) > 3CO2(g) + 4H2O(l)

What volume in liters of C3H7Cl is produced if 400.0g of C3H8 (propane) reacts with excess chlorine gas according to the equation C3H8+ Cl2 > C3H7Cl+HCl

Propane, C3H8, is a common fuel gas. Use the following to calculate the grams of propane you would need to provide 369 kJ of heat. C3H8 (g) + 5O2 (g) > 3CO2 (g)+ 4H2O (g) ; Delta H = 2043kJ

Propane, C3H8, is a common fuel gas. Use the following to calculate the grams of propane you would need to provide 383 kJ of heat. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔH = −2043 kJ

Many home barbeques are fueled with propane gas C3H8. What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9L of propane (approximate contents of one 5gallon tank)? Assume that the density of the liquid propane in the tank is

Propane (C3H8) burns in oxygen to produce carbon dioxide and water vapor. The balance equation for this reaction is C3H8 + 5O2 > 4H20 + 3CO2. What volume of carbon dioxide id produced when 2.8 L of oxygen are consumed? Here are the steps for solving

Q3: In the combustion reaction of 149g of propane(C3H8) with excess oxygen, what volume of carbon dioxide(CO2) is produced at STP? (note: balance the reaction first) C3H8 + O2 3CO2 + H2O

C3H8 + 5O2 > 3CO2 + 4H2O 22 moles of propane (C3H8) react with 200 moles of oxygen gas. how many moles of the non limiting reactant remain?

The combustion of 75.5 liters of 2 propane (c3h6)with 95.5 liters of oxygen gas is extremely exothermic. What is the maximum amount of water (in grams) to be made from this and how much of the nonlimiting reactant is unused at the end (in liters)?

Propane fuel is used in BBQs. Use the following reaction to determine how many moles of oxygen gas are needed to react with 1.6 moles of propane gas. C3H8(g)+5O2(g) > 4H2O(g)+ 3CO2(g)


The combustion of propane and oxygen produces carbon dioxide and water. What mass of water is produced from the combustion of 10.4g of propane, C3H8

4. Suppose that an excess of propane, C3H8 , burns in 320 g of oxygen, How many moles of water will be formed? C3H8 + 5 O2 > 3 CO2 + 4 H2O (1 point) 6.02 E 23 moles 1600 moles 4.0 moles 8.0 moles

how many liters of oxygen will react with 124.5 liters of propane

1. How many liters of carbon are produced at STP when 295g of methane gas (C3H8) is reacted with excess oxygen? The other products is water vapor. Write out a balanced equation. My answer: C3H8+O—> CO3+OH8?

Write a balanced equation for the combustion of gaseous propane (C3H8), a minority component of natural gas, in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water. I answered C3H8 + 5O2 = 3CO2 + 4H2O but it was wrong,

Propane (C3H8) burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is 103.9

How many liters of oxygen are necessary to burn 30.4 liters of ethyl alcohol (C2H5OH)? (Assume complete combustion)

Propane (C3H8) + oxygen> carbon dioxide + water how many grams of carbon dioxide are produced from the reaction of 35.2 grams of propane?

How much oxygen would be needed to completely burn 250g of propane?

If 2.33 L of propane (C3H8) at 24oC and 67.2 kPa is completely burned in excess oxygen, how many moles of carbon dioxide will be produced? a. Write a balanced equation for the reaction. b. Use stoichiometry to find the volume of carbon dioxide. c. Use the


Upon the combustion of propane, C3H8, 150. g of propane was reacted with excess oxygen gas. A. Determine the limiting reactant if the water is the product of interest. B. Determine the number of grams of water produced. C. Calculate the number of grams of

So I have the balanced equation: c3H8 +502 = 3C02 +4H20 Question: At STP propane (C3H8) burns in oxygen to form 2.15L of carbon dioxide and water. So I've got 2.15 L x 1 mole /22.4 L But when I try to do the mole ratio, I don't know what to do since the

Determine the mass of carbon dioxide that will be formed when 131.0 g of propane (C3H8) is reacted with 32 g of oxygen (O2) C3H8 + 5O2 > 3CO2 + 4H2O I got O2 as my limiting reagent. Then I used the mol of that which is 1 mol to find the mol of CO2

Use the following data 2C(s) + 4H2(g) > C3H8(g) DH= 103.85 kJ/molrxn C(s) + O2(g) > CO2(g) DH= 393.51 kJ/molrxn H2(g) + 1/2O2(g) > H2O(g) DH= 241.82 kJ/molrxn to calculate the heat of combustion of propane, C3H8 C3H8(g) + 5O2(g) 3CO2(g)

What mass of carbon dioxide will be produced when 0.250 mol of propane(C3H8) reacts with 25.0 g of oxygen? Write a balanced equation first.

The complete combustion of propane, C3H8(g), is represented by the equation: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH° = 2220 kJ

I am still not quite grasping how to complete this problem: Posted by K on Sunday, October 14, 2007 at 6:43pm. Many home barbeques are fueled with propane gas C3H8. What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9L of

when propane gas C3H8, is burned with oxygen, the products are carbon dioxide and water. Write an unbalanced formula equation for the reaction.

Calculate the energy released per gram of propane when it is burned in a combustion reaction. The chemical formula for propane is C3H8.

Calculate the number of grams of propane (C3H8) consumed if 17.7 g of water is produced according to the reaction: C3H8(g)+5O2(g)=3CO2(g)+4H2O(g)


How many grams of propane (C3H8) must be burned to release 3600kJ of energy? Standard Heat of combustion for Propane= 2220 kJ/Mole

A calorimeter consists of an interior metal bomb (container) surrounded by 2.22 kg of water all contained within an insulated exterior wall. A sample of propane, C3H8, weighing 6.89g, was burned in the calorimeter with excess oxygen. As a result of the

from the equation : c3h8+5O2=3CO2+4H20 HOW MANY GRAMS OF H2O CAN BE PRODUCED FROM THE REACTION OF 8.5X10^22 MOLECULES PROPANE GAS, C3H8

Calculate the partial pressure (in atm) of propane in a mixture that contains equal weights of propane (C3H8) and butane (C4H10) at 18°C and 746 mmHg

Calculate the mass of water formed by the complete reaction of 572 g of propane (C3H8) with excess oxygen. (Write a balanced equation.) Answer in units of g.

A propane gas (C3H8) heater burns propane at a rate of 500 grams per hour. a) What is the oxygen consumption rate? (in g O2/hr.) b) If the heater uses a blower to provide outside air (0°C, 1 atm) for combustion, what is the minimum air flow rate the

Propane reacts with oxygen in a combustion reaction. What volume of carbon dioxide gas is formed when 20 L of propane are reacted with 55.7 L of oxygen?

heat of combustion of propane c3h8, 2220KJ/mol. the specific heat of copper is 0.385 J/g*C. How many grams of propane must be burned to raise the temperature of a 10.0kg block of copper from 25.0 C to 65.0 C,assuming none of the heat is lost to the

The combustion of propane (C3H8)produces CO2 and H20: C3H8(g)+5O2(g) 3CO2(g)+4H2O(g) Calculate the mass, in grams, of H2O that will be produced if 2.5 mol of O2 is consumed.

The combustion of propane (C3H8)produces CO2 and H20: C3H8(g)+5O2(g) 3CO2(g)+4H2O(g) Calculate the mass, in grams, of H2O that will be produced if 2.5 mol of O2 is consumed.


What mass of propane (C3H8) is needed to produce 346g carbon dioxide in the following reaction? C3H8(g)+5O2(g)>3CO2(g)+4H2O(g) A. 68.8gS B. 3.07gS C. 13.5gS D. 41.0gS

Calculate the partial pressure of propane in a mixture that contains equal numbers of moles of propane (C3H8) and butane (C4H10) at 20 °C and 616 mmHg. (R=0.082 Latm/K mol)

Calculate the partial pressure of propane in a mixture that contains equal numbers of moles of propane (C3H8) and butane (C4H10) at 20 °C and 616 mmHg. (R=0.082 Latm/K mol)

Calculate the partial pressure of propane in a mixture that contains equal numbers of moles of propane (C3H8) and butane (C4H10) at 20 °C and 616 mmHg. (R=0.082 Latm/K mol)

Calculate the partial pressure of propane in a mixture that contains equal numbers of moles of propane (C3H8) and butane (C4H10) at 20 °C and 505 mmHg. (R=0.082 Latm/K mol)

Calculate the partial pressure of propane in a mixture that contains equal numbers of of moles of propane (C3H8) and butane (C4H10) at 20 degrees C and 844 mmHg. (R=0.082 Latm/K mol)

Propane is used in BBQs and burns according to the following equation: C3H8 + 5O2 > 3CO2 + 4H2O. If 2.2 moles of carbon dioxide are produced, how many moles of oxygen gas reacted?

Write a balanced chemical equation for the reaction for propane C3H8 burning in oxygen to for carbon dioxide and water vapor

Consider the combustion of propane: C3H8 + 5CO2 > 3CO2 + 2H20. Delta H = 2221 kJ. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 60.% efficient?

when 2.13 moles of C3H8 burn in excess oxygen, how many moles of CO2 will be formed? Assume this is a complete combustion


1) Calculate the volume of air at 30 degrees C and 1.00 atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O2 by volume. 2) Assuming all of the heat evolved in burning 30.0 g of propane is transferred to 8.00 kg of

How many moles of carbon dioxide would be produced if 0.28 moles of propane, C3H8, were combusted? C3H8 + 5 O2 > 3 CO2 + 4 H20

Hank Hill loves everything about gas propane, C3H8. One day his son Bobby asks him the following set of questions about propane. Hank hems and haws for a few moments and finally tells his son he'll get back to him with answers but he has to mow the lawn

the heat of combustion of propane is 5.47MJ/mol. there is 1.50kg of propane available to burn. how many litres of water could be heated from 18.0 degrees Celcius to 63.0 degrees Celcius using the heat from the burning propane. assume that all heat lost by

A 2.00 L flask is filled with propane gas (C3H8)at 1.00 atm and 15.0 Degrees Celsius. What is the mass of the propane in the flask?

A 2.00L flask is filled with propane gas(C3H8)at 1.00atm and 15C. What is the mass of propane in the flask?

A 2.00L flask is filled with propane gas(C3H8)at 1.00atm and 15C. What is the mass of propane in the flask?

How much heat is evolved when 5.00g of propane C3H8 burns completely. I got the formula down, now what? C3H8 + 5O2 > 3CO2 + 4H2O

Hank Hill loves everything about gas propane, C3H8. One day his son Bobby asks him the following set of questions about propane. Hank hems and haws for a few moments and finally tells his son he'll get back to him with answers but he has to mow the lawn

A 100 g piece of ice (solid water) at 0 °C melted to liquid water at 75.5 °C. If all the heat came from propane (C3H8) combustion, how many grams of propane Molar mass is 44.1'


A 3.24L flask is filled with propane gas (C3H8), at 1.00 atm and 13.5°C. What is the mass of the propane in the flask?

Many portable gas heaters and grills use propane, C3H8(g). Using enthalpies of formation, calculate the quantity of heat produced when 19.0g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.

Many portable gas heaters and grills use propane, C3H8(g). Using enthalpies of formation, calculate the quantity of heat produced when 17.0g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.

Many portable gas heaters and grills use propane, C3H8(g). Using enthalpies of formation, calculate the quantity of heat produced when 15.0g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.

how many liters of oxygen are required to react completely with 12.5 liters of hydrogen sulfide at stp?