How many grams of Butane (C4H10) must be burned to release 6375 KJ of heat?
Given: Molar mass of C4H10 =
here
So you need to find out how many moles of butane you need first:
6,375 kJ/mole / 2657 kJ = 2.40 moles
Multiply that times the molecular weight and you are done!
2.40 x 58 g/mole = 139 g answer is b)
Ah, burning butane, a classic! Now, to calculate how many grams of butane we need, we first need to figure out the molar mass of C4H10. Luckily, I have that information handy - the molar mass of C4H10 is approximately 58.12 grams per mole.
To determine the number of moles required, we'll use the formula: moles = energy released (in kJ) / molar enthalpy of combustion (in kJ/mol).
Now here's where things get a little tricky – the molar enthalpy of combustion depends on the reaction conditions. Could you provide more specific information?
The molar mass of C4H10 (butane) can be calculated by adding up the molar masses of each individual element:
(4 x molar mass of Carbon) + (10 x molar mass of Hydrogen)
= (4 x 12.01 g/mol) + (10 x 1.01 g/mol)
= 48.04 g/mol + 10.10 g/mol
= 58.14 g/mol
To calculate the number of grams of butane required to release 6375 kJ of heat, we need to use the following conversion factors:
1 mole C4H10 = 58.14 g
1 kJ = 1000 J
First, convert the heat released from kJ to J by multiplying it by 1000:
6375 kJ x 1000 J/kJ = 6,375,000 J
Next, use the molar mass of C4H10 to convert the amount of heat released in moles:
6,375,000 J x (1 mol C4H10 / 6375 kJ) = 1000 mol C4H10
Finally, convert the moles of butane to grams by using the molar mass of C4H10:
1000 mol C4H10 x 58.14 g/mol = 58,140 g
Therefore, 58,140 grams of butane must be burned to release 6375 kJ of heat.
To calculate the number of grams of Butane (C4H10) needed to release 6375 KJ of heat, we need to use the molar mass of C4H10 and the energy released per mole of Butane during combustion.
First, let's find the molar mass of Butane (C4H10). The molar mass is the sum of the atomic masses of all the atoms in one molecule of Butane.
The atomic mass of carbon (C) is approximately 12.01 grams/mole, and the atomic mass of hydrogen (H) is approximately 1.01 grams/mole.
Molar mass of C4H10 = (4 × atomic mass of carbon) + (10 × atomic mass of hydrogen)
= (4 × 12.01 g/mole) + (10 × 1.01 g/mole)
= 48.04 g/mole + 10.10 g/mole
= 58.14 g/mole
Now, using the concept of molar mass, we can determine the number of moles in 6375 KJ of heat. To do this, we need to know the molar enthalpy of combustion, which is the energy released per mole of Butane during combustion.
The molar enthalpy of combustion of Butane (C4H10) is approximately -2877 KJ/mol. The negative sign indicates that energy is released during the combustion process.
Using the following equation for energy:
Energy (KJ) = number of moles × molar enthalpy of combustion
Rearranging the equation to solve for the number of moles, we have:
Number of moles = Energy (KJ) ÷ molar enthalpy of combustion
Substituting the given values, we have:
Number of moles = 6375 KJ ÷ -2877 KJ/mol
Now we can calculate the number of moles of Butane:
Number of moles = -2.21 moles
Finally, we can calculate the mass of Butane in grams using the molar mass:
Mass (grams) = Number of moles × molar mass
Substituting the values, we have:
Mass (grams) = -2.21 moles × 58.14 g/mole
The negative sign indicates that the mass is an opposite quantity, so we take the absolute value and obtain:
Mass (grams) ≈ 128.23 grams
Therefore, approximately 128.23 grams of Butane must be burned to release 6375 KJ of heat.