0
To determine the moles of CO2 formed when 58 g of butane burns in oxygen, first, calculate the moles of butane using its molar mass. Then, use the stoichiometry of the balanced chemical equation to find the moles of CO2 formed, as per the ratio of the coefficients in the balanced equation.
What else can I help you with?
What compounds are found when you burn butane with a good supply of air?
Burning butane with a good supply of air will produce carbon dioxide, water vapor, and heat. The chemical reaction occurs as the butane (C4H10) combines with oxygen (O2) to form carbon dioxide (CO2) and water (H2O) through combustion.
How many moles of O2 are needed to burn 1.50 moles of C8H18?
The balanced equation for the combustion of C8H18 is: C8H18 + 12.5O2 -> 8CO2 + 9H2O From the equation, you need 12.5 moles of O2 to burn 1 mole of C8H18. So, to burn 1.50 moles of C8H18, you would need 1.50 x 12.5 = 18.75 moles of O2.
Butane burns in oxygen to produce magnesium nitrate an water?
no thats completely stupid. butane reacts with oxygen to produce carbon dioxide and water
How many moles of O2 are needed to burn 10 moles of Mg?
A. A balance chemical equation of burning of ethene is C2H4 + 3O2 ____ 2CO2 + 2H2O now according to balance chemical equation 1 mole of ethene burn by using 3 moles of oxygen so to burn 10 moles of ethene 3 x 10 30 moles of oxygen will be required.
How may grams of oxygen are required to burn 13.50 grams of acetylene?
To burn 1 mole of acetylene (C2H2), 3 moles of oxygen (O2) are required. The molar mass of acetylene is 26.04 g/mol and of oxygen is 32.00 g/mol. First, convert 13.50g acetylene to moles, calculate the moles of oxygen required, and then convert back to grams to find the mass of oxygen needed.
How many moles of co2 form when 58.0 g of butane c4h10 burn oxygen?
4 moles
How many moles of CO2 form when 58 grams of butane C4H10 burn in oxygen?
The answer is 3,99 moles of carbon dioxide.
How many moles of CO2 form when 58.0 g of butane C4H10 burn in oxygen?
For the combustion of butane C4H10, the balanced chemical equation is: 2C4H10 + 13O2 -> 8CO2 + 10H2O. First, calculate the moles of butane: 58.0 g / 58.12 g/mol = 1 mole. From the balanced equation, 2 moles of butane produce 8 moles of CO2, so 1 mole of butane will produce 4 moles of CO2.
How many grams of oxygen are required to burn 4.8 mol of butane?
The balanced equation for the reaction is 2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O. This shows that 13 moles of diatomic oxygen are required to burn 2 moles of butane. By proportionality, (4.8/2)13 or 31.2 moles of oxygen are required to burn 4.8 moles of butane. This corresponds to 31.2(32) or 1.0 X 103 grams of oxygen.
How many moles of co2 form when 58 grams of butane burn in oxygen?
The answer is 3,99 moles of carbon dioxide.
What compounds are found when you burn butane with a good supply of air?
Burning butane with a good supply of air will produce carbon dioxide, water vapor, and heat. The chemical reaction occurs as the butane (C4H10) combines with oxygen (O2) to form carbon dioxide (CO2) and water (H2O) through combustion.
How many moles of O2 are needed to burn 1.50 moles of C8H18?
The balanced equation for the combustion of C8H18 is: C8H18 + 12.5O2 -> 8CO2 + 9H2O From the equation, you need 12.5 moles of O2 to burn 1 mole of C8H18. So, to burn 1.50 moles of C8H18, you would need 1.50 x 12.5 = 18.75 moles of O2.
How many moles of oxygen are needed to burn 7.0 mols of phosphorus?
8,75 moles of oxygen are needed.
How many moles of O2 are needed to burn 1.35mol of C8H18?
16,875 moles of oxygen are needed.
Butane burns in oxygen to produce magnesium nitrate an water?
no thats completely stupid. butane reacts with oxygen to produce carbon dioxide and water
How many moles of O2 are needed to burn 10 moles of Mg?
A. A balance chemical equation of burning of ethene is C2H4 + 3O2 ____ 2CO2 + 2H2O now according to balance chemical equation 1 mole of ethene burn by using 3 moles of oxygen so to burn 10 moles of ethene 3 x 10 30 moles of oxygen will be required.
How may grams of oxygen are required to burn 13.50 grams of acetylene?
To burn 1 mole of acetylene (C2H2), 3 moles of oxygen (O2) are required. The molar mass of acetylene is 26.04 g/mol and of oxygen is 32.00 g/mol. First, convert 13.50g acetylene to moles, calculate the moles of oxygen required, and then convert back to grams to find the mass of oxygen needed.
