Answer:
A
Explanation:
Volume will help you determine whether is a solid or a liquid.
Have a great day
Answer:
Explanation:
Formula of percent composition:
% X = ( mass of element in compound / total mass of compound ) × 100
11) Al₂O₃
Al = 27 g/mol
O = 16 g/mol
%Al = (54 / 101.96) × 100
%Al = 52.9%
%O = (48 / 101.96) × 100
%O = 47.1%
12) C₅H₅O₅
C = 12 g/mol
H = 1 g/mol
O = 16 g/mol
C% = (60 / 145 ) × 100
C% =41.4%
H% = (5 / 145 ) × 100
H% =3.4%
O% = (80 / 145 ) × 100
O% = 55.2%
13) BaBr₂
Ba = 137.3 g/mol
Br =79.9 g/mol
Ba% = (137.3 / 297.14) × 100
Ba% = 46.2%
Br% = (159.8/ 297.14) × 100
Br% = 53.8%
14) Fe₃(PO₃)₂
Fe = 55.8 g/mol
P = 31 g/mol
O = 16 g/mol
Fe = (167.4/325.48) × 100
Fe = 51.43%
P = (62/325.48) × 100
P = 19.05%
O = (96 /325.48) × 100
O = 29.49%
The gas is ignited (I think) and combustion happens where the gasoline turns into gas (the state of being) and expands, pushing something and making the blades turn so
from stationary to explosive so potentioal to kenetic
Answer :
(1) The limiting reactant is the reactant that is completely consumed in a chemical reaction. → True
(2) The reactant in excess is any reactant that occurs in a quantity greater than that is required to completely react with the limiting reactant. → True
(3) The amount of product can be calculated based on the amount of limiting reactant. → True
Explanation :
Excess reagent : It is defined as the reactants not completely used up in the reaction. The given moles are more than the required moles.
Limiting reagent : It is defined as the reactants completely used up in the reaction. The given moles are less than the required moles.
Theoretical yield : It is calculated from the amount of the limiting reagent present in the reaction.
Actual yield : It is experimentally determined.
All the given statements are true.