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a_sh-v [17]
3 years ago
11

Determine how many grams of co2 are produced by burning 4.37 g of c4h10.

Chemistry
1 answer:
Flura [38]3 years ago
6 0
Combustion of hydrocarbons is when  C and H containing compounds are burnt in O₂
the balanced chemical reaction for combustion of C₄H₁₀ (butane) is as follows;
2C₄H₁₀ + 13O₂ ---> 8CO₂ + 10H₂O
the stoichiometry of C₄H₁₀ to CO₂ is 2;4, simplified ratio is 1:2
this means that for every 1 mole of butane used up,4 moles of CO₂ are formed
molar mass of butane - (12 g/mol *4) + (1 g/mol * 10) = 58 g/mol
58 g of butane      -  1 mol 
Therefore 4.37 g of butane - 1/58 g/mol * 4.37g = 0.075 mol
1 mol of butane forms --> 4 mol of CO₂
Therefore 0.075 mol of butane forms = 4 x 0.075 mol = 0.3 mol of CO₂
molar mass of CO₂ = 44 g/mol
mass of CO₂ formed = 0.3 mol * 44 g/mol = 13.2 g of CO₂ is formed 
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A 25 gram(m) metal ball is heated to 200C(delta T) with 2330 Joules(q) of energy. What is the specific heat of the metal?
Dominik [7]

Answer:

The specific heat of the metal is 0.466 \frac{J}{g*C}

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

The equation that allows calculating heat exchanges is:

Q = c * m * ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case:

  • Q= 2330 J
  • c= ?
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Replacing:

2330 J= c*25 g* 200 °C

Solving:

c=\frac{2330 J}{25 g* 200 C}

c=0.466 \frac{J}{g*C}

<u><em>The specific heat of the metal is 0.466 </em></u>\frac{J}{g*C}<u><em></em></u>

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