The empirical formula can be C₄H₈ or CH₃-CH=CH-CH₃.
Explanation:
As the number of moles of each element is already given ,then there is no need of further calculations. We can get the empirical formula by writing the moles of each element in its subscript position. As empirical formula is one of the simplest way to represent any chemical compound. So the given compound can be written as CₓHₙ. Here x and n are the number of moles of carbon and hydrogen present in the compound.
Since it is stated as the 4 moles of Carbon and 8 moles of hydrogen is present and it is known that each carbon can have maximum four single bond with its neighbors, so the empirical formula can be written as
C₄H₈ or CH₃-CH=CH-CH₃
Thus, the empirical formula can be C₄H₈ or CH₃-CH=CH-CH₃.
Answer:
W = 278.64375 Joules
Explanation:
The information given in this problem are;
Initial volume = 0L
Final volume = 2.50L
ΔV = 2.50 - 0 = 2.50 L
External pressure, P = 1.10 atm
Work = ?
These parameters are related by the equation;
w = - P ΔV
W = - (1.10 )(2.50)
W = 2.75 L atm
Upon conversion to joules;
1 liter atmosphere is equal to 101.325 joule
W = 278.64375 Joules
Carbon is more electronegative
Answer:
Explanation:
We are given this compound with the formula: C₃H₂O
According the subscripts, 1 molecule contains 3 carbon atoms, 2 hydrogen atoms, and 1 oxygen atom.
We can make a ratio. There are 3 carbon atoms for every 1 molecule of C₃H₂O.
Since we want to calculate the number of atoms in 200 molecules, we can multiply the ratio by 200.
200 molecules of C₃H₂O contains 600 atoms of carbon.
Answer:
Kindly check the explanation section.
Explanation:
From the description given in the question above, that is '' H subscript f to the power of degree of the reaction" we have that the description matches what is known as the heat of formation of the reaction, ∆fH° where the 'f' is a subscript.
In order to determine the heat of formation of any of the species in the reaction, the heat of formation of the other species must be known and the value for the heat of reaction, ∆H(rxn) must also be known. Thus, heat of formation can be calculated by using the formula below;
∆H(rxn) = ∆fH°( products) - ∆fH°(reactants).
That is the heat of formation of products minus the heat of formation of the reaction g specie(s).
Say heat of formation for the species is known as N(g) = 472.435kj/mol, O(g) = 0kj/mol and NO = unknown, ∆H°(rxn) = −382.185 kj/mol.
−382.185 = x - 472.435kj/mol = 90.25 kJ/mol