If I made no mistake in calculation, the given answer must be correct...(tried my best)
elements : carbon hydrogen oxygen Fluorine
composition [C] 24 3 16 57
M r 12 1 16 19
(divide C by Mr) 2 3 1 3
(Divide by smallest value) 2 3 1 3
(smallest value = 1...so all value remained constant)
Empirical formula : C2H3OF3
if molar mas = 100 g per mole, then
first step calculate Mr. of empirical formula: [= 100]
Them molecular formula = empirical formula
Hello There!
Conduction is the transfer of heat from one particle of matter to another.
“I Have 3 Examples Of Convection Provided Below”
“A Pot Sitting On A Hot Burner”
“Picking Up A Hot Cup Of Coffee”
“Feet On Hot Sand”
Answer:
- 20 J
Explanation:
Heat of Reaction = Heat of Products - Heat of Reactants
From the graph;
Heat of Products = 10
Heat of Reactants = 30
Heat of Reaction = 10 - 30 = -20 J
Answer:
Approximately 
grams.
Explanation:
Let 
represent the number of grams of aluminum iodide required to yield that 73.75 grams of aluminum.
In most cases, the charge on each aluminum ion would be +3 while the charge on each iodide ion would be -1. For the charges to balance, there needs to be three iodide ions for every aluminum ion. Hence, the empirical formula for aluminum iodide would be 
.
How many moles of formula units in that grams of ? Start by calculating its formula mass 
. Look up the relative atomic mass of aluminum and iodine on a modern periodic table:
.
.
Since there's one aluminum ion in every formula unit,
.
How many grams of aluminum would that be?
.
However, since according to the question, the percentage yield (of aluminum) is only 
. Hence, the actual yield of aluminum would be:
.
Given that the actual yield is 73.75 grams,
.
.
