2C3H7OH(l) + 9O2(g) → 8H2O(g) + 6CO2(g)
ΔHreaction = 1,830 kJ/mol
Calculate the enthalpy of combustion for 55.9g isopropanol given the molecular weight of isopropanol is 60.096 g/mol.

850.95 kj

Explanation:

Given data:

ΔH of reaction = 1830 kj/mol

Enthalpy of combustion for 55.9 g of isopropanol = ?

Solution:

Number of moles of isopropanol:

Number of moles = mass / molar mass

Number of moles = 55.9 g/ 60.096 g/mol

Number of moles =0.93 mol

1830 kj heat is produced when 2 mole of isopropanol react.

For one mole:

1830 kj/2 = 915 kj/mol

For 0.93 mol

0.93 mol × 915 kj/mol = 850.95 kj

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

they all get energy from eating other animals, dead animals to be more precise.

hienas tends to steal pray from other animals. crows and vultures tend to eat dead animals and leftovers.

hope it ,

bioteacher101