Answer:
I think the answer would be 'testable'.
Answer:
C
Explanation:
Think of 'exo' as exit and 'thermic' as relating to thermal energy/ heat. Thus, an exothermic release thermal energy as the reaction proceeds.
In an exothermic reaction, the total energy of the products is lesser than that of the reactants and ΔH (change in energy) is less than zero.
When heat is absorbed as the reaction proceeds, the chemical reaction is an endothermic reaction.
You divided them both by 108 to get 125/32. you cant just leave it like that though. You turn it into a mixed number. So the correct answer is 3 29/32
Answer:
40.68 % C
23.73 % N
8.47% H
27.12% O
Explanation:
The mass percent of an element X in a compound is calculated as the molar mass (MM) of X multiplied by the number of atoms of X in the compound, divided into the molecular weight (MW) of the compound, as follows:
mass percent of X = (MM(X) x number of atoms of X)/MW compound x 100
Thus, we first calculate the MW of acetamide (C₂H₅NO) by using the molar mass of the chemical elements C, H, N and O:
MW(C₂H₅NO) = (12 g/mol C x 2) + (1 g/mol H x 5) + 14 g/mol N + 16 g/mol O = 59 g/mol
Now, we can calculate the mass percent of each element (C, H, N, O) in C₂H₅NO:
- Mass percent of C (2 atoms of C in 1 molecule of C₂H₅NO):
% mass C = (12 g/mol x 2)/(59 g/mol) x 100 = 40.68 %
- Mass percent of N (1 atom of N in 1 molecule of C₂H₅NO):
% mass N = (14 g/mol x 1)/(59 g/mol) x 100 = 23.73 %
- Mass percent of H (5 atoms of H in 1 molecule of C₂H₅NO):
% mass H = (1 g/mol x 5)/(59 g/mol) x 100 = 8.47 %
- Mass percent of O (1 atom of O in 1 molecule of C₂H₅NO):
% mass O = (16 g/mol x 1)/(59 g/mol) x 100 = 27.12 %
The sum of the mass percents has to be equal to 100%:
40.68 % C + 23.73 % N + 8.47% H + 27.12% O = 100%
Answer:
Explanation:
1. Mass of zinc
The density of zinc is 7.14 g/cm³
D = m/V
2. Volume of aluminium
The density of aluminium is 2.60/cm³.