t takes 572 kJ of energy to decompose 2.00 mol of liquid water. How much energy does it take to decompose 54.0 mol of water?
2H2O(l)+572kJ→2H2(g)+O2(g)
572 kJ x (54.0/2.00) = ? kJ
To find the energy required to decompose 54.0 moles of water, we can set up a proportion using the given information.
According to the equation, it takes 572 kJ to decompose 2.00 moles of water:
2 moles H2O -> 572 kJ
We can set up the proportion as follows:
2 moles H2O x kJ
------------- = -------------
572 kJ 54.0 moles H2O
To solve for x, we can cross-multiply and divide:
2 moles H2O * 54.0 moles H2O = 572 kJ * x kJ
108 moles H2O = 572 kJ * x kJ
Dividing both sides by 572 kJ:
108 moles H2O / 572 kJ = x kJ
0.1888 moles H2O = x kJ
Therefore, it would take approximately 0.1888 kJ of energy to decompose 54.0 moles of water.
To find out how much energy it takes to decompose 54.0 mol of water, we can use a proportion based on the given information.
First, let's set up the proportion:
Energy (kJ) = (Number of moles of water / Number of moles of water in the given scenario) * Energy in the given scenario
Given:
Number of moles of water in the given scenario = 2.00 mol
Energy in the given scenario = 572 kJ
Let's plug in the values into the proportion:
Energy (kJ) = (54.0 mol / 2.00 mol) * 572 kJ
Now, let's calculate the energy:
Energy (kJ) = (27) * 572 kJ
Energy (kJ) = 15,444 kJ
Therefore, it would take 15,444 kJ of energy to decompose 54.0 mol of water.