Calculate the maximun=m mass of ethanol that can be made from 5.6 tonnes of ethen
ether ==> ethanol
Balance the equation.
mols ether = tonnes/molar mass (OK, this isn't mols but a tonne-mole but we will be consistent throughout so this is ok. If you don't do this you must convert tonnes to grams in this step and from grams back to tonnes in the last step).
Using the coefficients in the balanced equation, convert tonne-mols ether to tonne-moles ethanol).
Now convert that to tonnes ethanol by multiplying by molar mass ethanol.
The decomposition of NO2 at room temperature exhibits the following variation in concentration with time:
The concentration of NO2 is expressed in mol/liter, while time is expressed in seconds.
[NO2] ln[NO2] 1/[NO2] Time (s)
0.0831 -2.4877 12.03 0
0.0666 -2.7091 15.02 4.2
0.0567 -2.8700 17.64 7.9
0.0487 -3.0221 20.53 11.4
0.0441 -3.1213 22.68 15.0
a. Express the rate of decomposition of NO2 as a function of the concentration of NO2 and determine the order of reaction. (numerical response only: 1 = 1st order, 1.5 = three halves order, 2 = 2nd order, etc.)
2 - correct
b. Determine the value of the rate constant.
0.71 - correct
To calculate the maximum mass of ethanol that can be made from 5.6 tonnes of ethene, we need to know the balanced chemical equation for the reaction converting ethene to ethanol. The balanced equation for the reaction is:
C2H4 + H2O -> C2H5OH
From the balanced equation, we can see that 1 mole of ethene (C2H4) reacts with 1 mole of water (H2O) to produce 1 mole of ethanol (C2H5OH). Now, we need to find the molar mass of ethene and ethanol.
The molar mass of ethene (C2H4):
C: 12.01 g/mol
H: 1.01 g/mol (there are 4 hydrogens in ethene)
Molar mass of ethene = (2 * 12.01 g/mol) + (4 * 1.01 g/mol) = 28.05 g/mol
The molar mass of ethanol (C2H5OH):
C: 12.01 g/mol (there are 2 carbons in ethanol)
H: 1.01 g/mol (there are 6 hydrogens in ethanol)
O: 16.00 g/mol
(additional note on balances O we have [there are 1 oxygen in ethanol])
Molar mass of ethanol = (2 * 12.01 g/mol) + (6 * 1.01 g/mol) + 16.00 g/mol = 46.07 g/mol
Now, let's calculate how many moles of ethene are in 5.6 tonnes. To do this, we'll use the molar mass of ethene.
Moles of ethene = Mass of ethene / Molar mass of ethene
Moles of ethene = 5.6 tonnes * 1000 kg/tonne / 28.05 g/mol (convert tonnes to kilograms)
Simplifying,
Moles of ethene = 200,000 g / 28.05 g/mol = 7121.97 mol
Since the reaction is 1:1, the maximum amount of ethanol produced will also be 7121.97 moles.
Finally, we'll calculate the mass of this amount of ethanol using its molar mass.
Mass of ethanol = Moles of ethanol * Molar mass of ethanol
Mass of ethanol = 7121.97 mol * 46.07 g/mol ≈ 328,053 g
So, the maximum mass of ethanol that can be made from 5.6 tonnes of ethene is approximately 328,053 grams (or 328.05 kg).