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The reaction can be described using the equation: 2C2H25O24CO22H2O. How much C2H2is needed to react with 68.1 g of O2to produce

Sophie [7]

Answer:

22.13g

Explanation:

We'll begin by writing a balanced equation for the reaction. This is illustrated below:

2C2H2 + 5O2 —> 4CO2 + 2H2O

Next, we'll calculate the mass of C2H2 and O2 that reacted from the balanced equation. This is illustrated below:

Molar Mass of C2H2 = (12x2) + (2x1)

= 24 + 2 = 26g/mol

Mass of C2H2 that reacted from the balanced equation = 2 x 26 = 52g

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 that reacted from the balanced equation = 5 x 32 = 160g

Now, we can obtain the mass of C2H2 that will react with 68.1g of O2 as follow:

From the balanced equation above,

52g of C2H2 reacted with 160g of O2.

Therefore, Xg of C2H2 will react with 68.1g of O2 i.e

Xg of C2H2 = (52x68.1)/160

Xg of C2H2 = 22.13g

Therefore, 22.13g of C2H2 is needed to react with 68.1g of O2

8 0

3 years ago

Ethylene oxide (EO) is prepared by the vapor-phase oxidation of ethylene. Its main uses are in the preparation of the antifreeze

Rashid [163]

Answer:

a. Δ $H^0_{rxn} = -108.0\frac{kJ}{mol}$

b. 320.76° C

Explanation:

a.)

we can solve this type of question (i.e calculate Δ $H^0_{rxn}$ , for the gas-phase reaction ) using the Hess's Law.

Δ $H^0_{rxn}$ = $E_{product} deltaH^0_{t}-E_{reactant} deltaH^0_{t}$

Given from the question, the table below shows the corresponding Δ $H^0_{t}(kJ/mol)$ for each compound.

Compound $H^0_{t}(kJ/mol)$

Liquid EO -77.4

$CH_4_(g_)$ -74.9

$CO_(g_)$ -110.5

If we incorporate our data into the above previous equation; we have:

Δ $H^0_{rxn}$ = (-110.5 kJ/mol + (-74.9 kJ/mol) ) - (-77.4 kJ/mol)

= $-108.0 \frac{kJ}{mol}$

b.)

We are to find the final temperature if the average specific heat capacity of the products is 2.5 J/g°C

Given that:

the specific heat capacity (c) = 2.5 J/g°C

$T_{initial}$ = 93.0°C &

the enthalpy of vaporization (Δ $H^0_{vap}$ ) = 569.4 J/g

If, we recall; we will remember that; Specific Heat Capacity is the amount of heat needed to raise the temperature of one gram of a substance by one kelvin.

∴ the specific heat capacity (c) is given as = $\frac{Heat(q)}{mass*changeintemperature(T_{initial}-T_{final})}$

Let's not forget as well, that Δ $H^0_{vap}$ = $\frac{q}{mass}$

If we substitute Δ $H^0_{vap}$ for $\frac{q}{mass}$ in the above equation, we have;

specific heat capacity (c) = $\frac{deltaH^0_{vap}}{T_{final}-T_{initial}}$

Making ( $T_{final}- T_{initial}$ ) the subject of the formula; we have:

$T_{final}- T_{initial}$ = $\frac{delat H^0_{vap}}{specificheat capacity}$

$(T_{final}-93.0^0C)=\frac{569.4J/g}{2.5J/g^0C}$

$T_{final}=\frac{569.4J/g}{2.5J/g^0C}+93.0^0C$

= 227.76°C +93.0°C

= 320.76°C

∴ we can thereby conclude that the final temperature = 320.76°C

7 0

3 years ago

Consider a generic redox reaction?

vesna_86 [32]

The Nernst equation allows us to predict the cell potential for voltaic cells under conditions other than the standard conditions of 1M, 1 atm, 25°C. The effects of different temperatures and concentrations may be tracked in terms of the Gibbs energy change ΔG. This free energy change depends upon the temperature & concentrations according to ΔG = ΔG° + RTInQ where ΔG° is the free energy change under conditions and Q is the thermodynamic reaction quotient. The free energy change is related to the cell potential Ecell by ΔG= nFEcell

so for non-standard conditions
-nFEcell = -nFE°cell + RT InQ

or

Ecell = E°cell - RT/nF (InQ)

which is called Nernst equation.

5 0

3 years ago

how many milliliters of a stock solution of 2.00M KNO3 would you need to prepare 100.0mL of 0.150M KNO3?

larisa86 [58]

The answer is 7.5 ml

3 0

3 years ago

ATOMS WE LOVE ATOMS, answer this and get points , also thx for your help :)

LuckyWell [14K]

Answer:C because they have to I have the same mass before and after the equation.

Explanation:

HOPE THIS HELPED!! :) ;) <3<3