<h3><u>Answer</u>;</h3>
C3H4O
<h3><u>Explanation;</u></h3>
Empirical formula is the simplest formula of a compound;
Molar mass CO2 = 44.01
Mass of CO2 produced = 2.053 g
Mass of carbon in original sample = 12.01/44.01 × 2.053
= 0.5603g
Molar mass H2O = 18
Mass of H in original sample = 2/18 ×0.5601
= 0.0622 g
Thus; original sample contained 0.5603g C and 0.0622g H. The balance of the sample was O
Mass of O = 0.8715 - (0.5603 + 0.0622) = 0.249g
The mole ratio of C:H:O will be;
Moles C = 0.5603/12 = 0.0467
Moles H = 0.0622
Moles O = 0.249/16 = 0.01556
C:H:O = 0.0467:0.0622:0.01556
Divide through by 0.01556:
C:H:O = 3:4:1
Empirical formula is thus C3H4O
Answer:
The answer is
<h2>53.56 mL</h2>
Explanation:
The volume of a substance when given the density and mass can be found by using the formula
From the question
mass of rock = 316 g
density = 5.9 g/mL
The volume of the rock is
We have the final answer as
<h3>53.56 mL</h3>
Hope this helps you
Answer:
You can make Cake CAke Cake Cake and other stuff too Ig
Explanation:
<span>Answer
is: mass of burned butane is 11.6 g.</span>
Chemical reaction: 2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O.
m(butane)
= 50,0 g.
<span>
V(CO</span>₂) = 17,9 L.<span>
n(CO</span>₂) = V(CO₂) ÷
Vm.<span>
n(CO</span>₂) = 17,9 L ÷ 22,4 L/mol.<span>
n(CO</span>₂) = 0,8 mol.<span>
From chemical reaction n(CO</span>₂) :
n(C₄H₁₀) = 8 : 2.<span>
n(C</span>₄H₁₀) =
0,8 mol ÷ 4.<span>
n(C</span>₄H₁₀) =
0,2 mol.<span>
m(C</span>₄H₁₀) =
n(C₄H₁₀) · M(C₄H₁₀).<span>
m(C</span>₄H₁₀) =
0,2 mol · 58 g/mol.<span>
m(C</span>₄H₁₀) =
11,6 g.
