Answer:
Explanation:
Butane is the 4th member of alkane series. It has 4 carbon atoms.
First write a balanced equation for the combustion of butane as follows;
2C4H10 + 13O2 ===> 8CO2 + 10H2O
from the balanced equation,
2C4H10 weigh 2[(12 x 4) + (1 x 10)]
=2(48 + 10)
= 116g
13O2 weigh 13(16 x 2)
=13 x 32
= 416g
8CO2 weigh 8[ 12+ (16 x 2)]
8 x (12 + 32)
352g
From the equation, 116g of buthane produced 352g of carbon dioxide
10g of buthane will produce 10×116÷352 =
Cohesion holds hydrogen bonds together to create surface tension on water. Since water is attracted to other molecules, adhesive forces pull the water toward other molecules.
Answer: Internal Temperatures. Similarly, the cardiovascular, integumentary (skin and associated structures), respiratory, and muscular systems work together to help the body maintain a stable internal temperature. If body temperature rises, blood vessels in the skin dilate, allowing more blood to flow near the skin's surface.
Explanation:
Answer:
% Yield = 81.4%
Explanation:
Based on the reaction:
C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O
<em>1 mole of C₈H₁₈ reacts with 25/2 moles of O₂ to produce 8 moles of CO₂</em>
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To solve this question we must, as first, find limiting reactant. With limiting reactant we can find theoretical yield of CO₂. Percent yield is defined as:
% Yield = Actual yield (917g CO₂) / Theoretical Yield * 100
For a complete reaction of 4.00 moles of C₈H₁₈ are required:
4.00moles C₈H₁₈ * (25/2 moles O₂ / 1mol C₈H₁₈) = 50.0 moles of O₂
As there are just <em>40.0 moles, O₂ is limiting reactant</em>
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The theoretical yield of CO₂ from 40.0 moles of O₂ is:
40.0 moles O₂ * (8 moles CO₂ / 25/2 moles O₂) = 25.6 moles of CO₂
As molar mass of CO₂ is 44.01g/mol:
25.6 moles of CO₂ * (44.01g / mol) = 1126.7g of CO₂ is theoretical yield
And percent yield is:
% Yield = 917g / 1126.7g * 100
<h3>% Yield = 81.4%</h3>
