Answer:
The answer to your question is empirical formula = CH
molecular formula = C₆H₆
Explanation:
Data
Carbon 92.2%
Hydrogen 7.76%
Formula mass = 78.1 g
Process
1.- Express the percents as grams
Carbon 92.2 g
Hydrogen 7.76 g
2.- Convert the grams to moles
Carbon 12 g ---------------- 1 mol
92.2 g ------------- x
x = (92.2 x 1)/12
x = 7.68 moles
Hydrogen 1 g ------------------ 1 mol
7.76 g ------------- x
x = 7.76 moles
3.- Divide by the lowest number of moles
Carbon 7.68 / 7.68 = 1
Hydrogen 7.76 / 7.68 = 1.01
4.- Write the empirical formula
CH
5.- Calculate the molecular weight of the empirical formula
CH = 12 + 1 = 13
6.- Divide the molecular weight by the molecular weight of the empirical formula
78.1 / 13 = 6
7.- Write the molecular formula
6(CH) = C₆H₆
Answer:
(C) when bonds in food are broken, energy is released
Answer:
weight = mg
= 2 X 9.8 (g = 9.8m/s^2)
= 19.6 N is the correct answer
Answer:
C
Explanation:
A negative deltaH means that the reaction has to give up heat in order to happen. You have to treat deltaH as a reactant. So the question is do you need to add heat to the reactants to make the products. If you do, deltaH is plus.
Heat is required to make a solid go to a gas. deltaH is plus. A is not the answer.
A lot of heat is required for B (something like 400 Kj / mole. Like A, deltaH is plus and B is not the answer.
C: The liquid has to give up heat in order for the this reaction to take place. C is the answer.
D requires heat. It is not the answer.