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How many moles of oxygen are required to react with 5 moles of butane?
Assuming complete combustion of butane, you need 15 moles of oxygen to react with 5 moles of butane according to the balanced chemical equation: [ 2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O ]
If 5.50 mol of butane are reacted how many moles of water vapor are produced?
Each mole of butane, which has formula of C4H10, contains 10 moles of hydrogen atoms. If the butane is completely combusted, all of the hydrogen in the butane is converted in water, with the formula H2O. The amount of water vapor will accordingly be 5.50 X 10/2 = 27.5.
How many grams of water are needed to react with 0.373 mol of ethylene?
To react with 0.373 mol of ethylene (C2H4), you need an equal number of moles of water (H2O) based on the balanced chemical equation: C2H4 + H2O → C2H5OH This means you need 0.373 mol of water to react with 0.373 mol of ethylene. To convert moles to grams, you would multiply 0.373 mol by the molar mass of water (18.015 g/mol) to get the grams needed.
How many moles K are needed to react with 15 moles of Cl2?
H2 +Cl2---------------->2HCl Since H2 and Cl2 react in 1:1 mole ratio the number of moles of H2 reacting is equal to the number of moles of Cl2 which is equal to 0.213
How many grams of H2O are needed to react with 3.5 moles of ethylene?
63 g of water are needed.
How many grams of Oxygen are needed to completely react with 5.0 grams of butane in a butane lighter?
To calculate the grams of oxygen needed, you first need to balance the chemical equation for the combustion of butane. C₄H₁₀ + O₂ → CO₂ + H₂O. From the balanced equation, 2 moles of butane react with 13 moles of oxygen. One mole of butane is 58.12 g, and one mole of oxygen is 32 g. Therefore, 5.0 g of butane would require (5.0 g / 58.12 g/mol) * 13 moles of oxygen, which is approximately 1.12 grams of oxygen.
How many moles of oxygen are required to react with 5 moles of butane?
Assuming complete combustion of butane, you need 15 moles of oxygen to react with 5 moles of butane according to the balanced chemical equation: [ 2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O ]
If 5.50 mol of butane are reacted how many moles of water vapor are produced?
Each mole of butane, which has formula of C4H10, contains 10 moles of hydrogen atoms. If the butane is completely combusted, all of the hydrogen in the butane is converted in water, with the formula H2O. The amount of water vapor will accordingly be 5.50 X 10/2 = 27.5.
How many grams of water are produced when 2.5 mil oxygen reacts with hydrogen?
When 2.5 moles of oxygen react with hydrogen, they react in a 1:2 ratio to produce water. Therefore, 2.5 moles of oxygen will produce 5 moles of water. To convert moles to grams, you'll need to know the molar mass of water, which is approximately 18 grams/mol. So, 2.5 moles of oxygen will produce 90 grams (5 moles x 18 grams/mole) of water.
How many grams of CO react with .390 kg of Fe2O3?
Fe2O3 (s) + 3 CO (g) 🡪 2 Fe (s) + 3 CO2 (g) Calculate the number of grams of CO that can react with 250 g of Fe2O3. Calculate the number of grams of Fe and the number of grams of CO2 formed when 250 grams of Fe2O3 reacts.
When carbon is burned in the presence of oxygen the carbon and oxygen combine to prodon dioxide if you start w 6 grams of carbon and 16 grams of oxygen and they react completely how many grams of car?
the equation of this reaction is C + O2 = CO2 (s) (g) (g) according to this reaction 1mol of Carbon react with same number of moles of Oxygen. and this combination gives 1mol of CO2 as result. so first we have to find the number of moles in the weight we are going to use. 12 grams of carbon contains 1mol so 6 grams of carbon contains ( 1/12 )*6 = 0.5mol 32 grams of Oxygen contains 1mol 16 grams of Oxygen contains ( 1/36 )*16 = 0.5mol as 1mol of C react with 1mol of O2,0.5mol of C react with 0.5mol of O2. this produces equal number of moles (0.5mol) of CO2.
How many grams of oxygen are needed to react with 350 grams of iron to produce 500 grams of fe203?
The balanced chemical equation for the reaction between iron and oxygen to produce Fe2O3 is 4Fe + 3O2 -> 2Fe2O3. From the equation, we see that 3 moles of oxygen react with 4 moles of iron to produce 2 moles of Fe2O3. Therefore, to find the grams of oxygen needed, we need to calculate the molar mass of Fe2O3 and then determine the number of grams needed using the mole ratio from the balanced equation.
What volume of 6.0 M HCl is required to react with 10.0 grams of K2CO3?
First, calculate the number of moles of K2CO3 in 10.0 grams. Next, write and balance the chemical equation for the reaction between HCl and K2CO3. Use the stoichiometry of the balanced equation to determine the number of moles of HCl required to react with the moles of K2CO3. Finally, use the molarity of the HCl solution to calculate the volume needed.
How many grams of H3PO4 are produced when 10.0 moles of water react with an excess of P4O10?
1 mole of P4O10 reacts with 6 moles of water to produce 4 moles of H3PO4. Therefore, 10.0 moles of water will produce (10/6)*4 moles of H3PO4. To convert moles to grams, multiply the number of moles by the molar mass of H3PO4.
Does silicone react with butane?
No, silicone does not react with butane. Silicone is chemically inert, meaning it does not easily react or interact with other chemicals, including butane. This property makes silicone a popular choice for containing substances like butane.
How many grams of water are needed to react with 0.373 mol of ethylene?
To react with 0.373 mol of ethylene (C2H4), you need an equal number of moles of water (H2O) based on the balanced chemical equation: C2H4 + H2O → C2H5OH This means you need 0.373 mol of water to react with 0.373 mol of ethylene. To convert moles to grams, you would multiply 0.373 mol by the molar mass of water (18.015 g/mol) to get the grams needed.
How many grams of nitrogen dioxide must react with water to produce 5.00 x 1022 molecules of nitrogen monoxide?
To find the grams of nitrogen dioxide needed, first calculate the moles of nitrogen monoxide using Avogadro's number. Then, use the balanced chemical equation to determine the moles of nitrogen dioxide required. Finally, convert moles to grams using the molar mass of nitrogen dioxide.
