Test tubes, flasks, bunsen burners, random chemical equations
protons
there aint rlly an explanation tbh
Answer:
27,397.23 L would be needed for a successful trip.
Explanation:
The problem gives us <u>the density (ρ) of the fuel,</u> by telling us that there are 803 g of fuel in 1 L, in which case:
ρ=
The required mass of fuel is 2.2 * 10⁴ kg, we can convert this value into g:
2.2 * 10⁴ kg *
= 2.2 * 10⁷ g
We calculate the required volume (V), using the mass and density:

Thus 27,397.23 L would be needed for a successful trip.
Dissolves easily in water
Answer:
C₄H₈O₂.
Explanation:
- Firstly, we can calculate the no. of moles (n) of each component using the relation:
<em>n = mass/atomic mass,</em>
mol C = mass/(atomic mass) = (54.5 g)/(12.0 g/mol) = 4.54 mol.
mol H = mass/(atomic mass) = (9.3 g)/(1.0 g/mol) = 9.3 mol.
mol O = mass/(atomic mass) = (36.2 g)/(16.0 g/mol) = 2.26 mol.
- To get the empirical formula, we divide by the lowest no. of moles (2.26 mol) of O:
∴ C: H: O = (4.54 mol/2.26 mol) : (9.3 mol/2.26 mol) : (2.26 mol/2.26 mol) = 2: 4: 1.
<em>∴ Empirical formula mass of (C₂H₄O) = 2(atomic mass of C) + 4(atomic mass of H) + 1(atomic mass of O) =</em> 2(12.0 g/mol) + 4(1.0 g/mol) + (16.0 g/mol)<em> = 44.0 g/mol.</em>
∴ Number of times empirical mass goes into molecular mass = (88.0 g/mol)/(44.0 g/mol) = 2.0 times.
∴ The molecular formula is, 2(C₂H₄O), that is; <em>(C₄H₈O₂)</em>