Answer is C
A synthesis reaction looks like this:
A+ B → AB
Density is ratio of mass and volume.
therefore Density is equal to mass/ volume
but mass =3.60gand volume =1.8cm3
therefore density is equal to 3.60/1.8
density = 2.0gcm3
The question is incomplete, the complete question is;
A 31 g sample of a compound that contains only the elements C,H and N is completely burned in O2 to produce 44.0 g of CO2, 45.0 g of H2O, and 92.0 g of NO2. Determine the empirical formula of the compound.
Answer:
CH5N2
Explanation:.
Mass of C = 44.0g/44.0 g/mol = 1 mol * 1 = 1 mole of C
Mass of H = 45.0 g/18 g/mol = 2.5 moles * 2 = 5 moles of H
Mass of N = 92.0 g/46 g/mol = 2 moles * 1 = 2 moles of N
Dividing through by the lowest mole ratio;
1/1, 5/1, 2/1
1 : 5 : 2
Hence the empirical formula is;
CH5N2
Answer:
38,640g
Explanation:
Since the density is in g/mL, we have to convert 2.000 liters to mil-liters to be able to successfully use the formula of M=V*D. Convert liters to mil-liters and you should have 2000mL in which you can plug into the equation of M= 2000mL*19.32g/mL, mL cancels, and you're left with 38,640g (here the significant figures are already in check).
Answer:
a) 157.5 grams of aluminum.
b) 1 mol
c) 9 g
Explanation:
The reaction is :
As per balanced equation
a) 3 moles of hydrogen will be produced from two moles of aluminium.
The atomic mass of aluminium = 27
therefore
3X2 grams of hydrogen is produced from 2 X 27 grams of Al
1 gram of hydrogen will be produced from 
g
therefore 17.5 will be produced from = 9X 17.5 = 157.5 grams of aluminum.
b) as per balanced equation three moles or six gram of hydrogen is produced from 6 moles of NaOH.
Therefore 1 g of hydrogen will be produced from =
or 1 gram will be prepared from = 1 mole
c) from balanced equation three moles are produced from two moles of Al (27X2 = 54 g).
thus from 54 grams gives 6 grams of hydrogen
1 grams will give = 
