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shtirl [24]
3 years ago
11

O2 + 2C0-2CO2

Chemistry
1 answer:
andreev551 [17]3 years ago
5 0

Answer: 1. CO is the limiting reagent and O_2 is the excess reagent.

2. 2.91 g of excess reagent

3. 4.66 g of carbon dioxide produced.

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} CO=\frac{2.98g}{28g/mol}=0.106moles

\text{Moles of} O_2=\frac{4.62g}{32g/mol}=0.144moles

O_2+2CO\rightarrow 2CO_2  

According to stoichiometry :

2 moles of CO require = 1 mole of O_2

Thus 0.106 moles of CO will require=\frac{1}{2}\times 0.106=0.053moles  of O_2

Thus CO is the limiting reagent as it limits the formation of product and O_2 is the excess reagent.

Amount of excess reagent = ( 0.144-0.053) moles = 0.091 moles

Mass of excess reagent O_2=moles\times {\text {Molar mass}}=0.091moles\times 32g/mol=2.91g

As 2 moles of CO give = 2 moles of CO_2

Thus 0.106 moles of CO give =\frac{2}{2}\times 0.106=0.106moles  of CO_2

Mass of CO_2=moles\times {\text {Molar mass}}=0.106moles\times 44g/mol=4.66g

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As there are more moles of NaOH than moles of HCl, <em>HCl is limiting reactant and moles of reaction are moles of limiting reactant, </em><em>0.0635 moles</em>

<em />

Using the coffee-cup calorimeter equation we can find how many heat was released thus:

Q = C×m×ΔT

<em>Where Q is heat released, C is specific heat of the solution (4.18J/g°C), m is mass of solution (100g because there are 100mL of solution -50.0mL of HCl and 50.0mL of NaOH- and density is 1g/mL) and ΔT is change in temperature (8.49°C)</em>

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Now, change in enthalpy, ΔH, is equal to change in heat (As is released heat ΔH < 0) per mole of reaction, that is:

ΔH = Heat / mol of reaction

ΔH = -3548.8J / 0.0635 moles of reaction

<em>Negative because is released heat. </em>

ΔH = -55887J / mol

ΔH =

<h3>-55.9kJ/mol is the change in enthalpy of the reaction</h3>

<em />

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