Question

Be sure to answer all parts. The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. H2(g) + CO2(g) ⇌ H2O(g) + CO(g) Calculate ΔG o for the reaction. kJ/mol Calculate ΔG for the reaction when the partial pressures are PH2 = 0.27 atm, PCO2 = 0.82 atm, PH2O = 0.66 atm, and PCO = 1.18 atm.

Answer 1

When there is a balanced equation then:

H2 (g) + CO2 (g) ↔ H2O (g) + CO (g)

Further Explanation

a) first, to calculate ΔG ° for the reaction:

we will use this formula:

ΔG ° = -RT㏑Kp

when R is that the constant Rydberg = 8,314J / mol.K

and T is that the temperature at Kelvin = 2000 K

and Kp = 4.4

so, by substitution:

ΔG ° = - 8,314 * 2000 * ㏑4.4

= - 24624 J / mol = - 24.6 KJ / mol

b) to calculate ΔG so, we'll use this formula:

ΔG = ΔG ° + RT㏑Qp

So we first have to, to induce Qp from the reaction equation:

when Qp = product P / reactant

= PH2O * PCO / PH2 * PCO2

= (0.66 atm * 1.2 atm) / (0.25 * 0.78)

= 4.1

so with substitution:

ΔG = -24624 + 8,314 * 2000 * ㏑4.1

= -1162 J / mol = - 1.16 KJ / mol

A chemical reaction is a natural process that always produces interchange of chemical compounds. The initial compounds or compounds involved in the reaction are called reactants. Chemical reactions are usually characterized by chemical changes and will produce one or more products that usually have different characteristics from reactants.

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Chemical Reaction  brainly.com/question/12904248

Balanced Equation  brainly.com/question/12904248

Details

Grade: College

Subject: Chemistry

Keyword: chemical, equation, reaction

Answer 2

Answer:

For 1: The value of $\Delta G$ for the chemical equation is -24.636 kJ/mol

For 2: The value of $\Delta G$ for the chemical equation is -20.925 kJ/mol

Explanation:

For the given chemical equation:

$H_2(g)+CO_2(g)\rightleftharpoons H_2O(g)+CO(g)$

• For 1:

To calculate the $\Delta G$ for given value of equilibrium constant, we use the relation:

$\Delta G=-RT\ln K_p$      .....(1)

where,

$\Delta G$ = ? kJ/mol

R = Gas constant = $8.314J/K mol$

T = temperature = 2000 K

$K_p$ = equilibrium constant in terms of partial pressure = 4.40

Putting values in above equation, we get:

$\Delta G=-(8.314J/Kmol)\times 2000K\times \ln (4.40)\\\\\Delta G=-24636.12J/mol$

Converting this into kilo joules, we use the conversion factor:

1 kJ = 1000 J

So, -24636.12 J/mol = -24.636 kJ/mol

Hence, the value of $\Delta G$ for the chemical equation is -24.636 kJ/mol

• For 2:

The expression of $K_p$ for the given chemical equation is:

$K_p=\frac{p_{CO}p_{H_2O}}{p_{H_2}p_{CO_2}}$

We are given:

$p_{CO}=1.18atm\\p_{H_2O}=0.66atm\\p_{CO_2}=0.82atm\\p_{H_2}=0.27atm$

Putting values in above equation, we get:

$K_p=\frac{1.18\times 0.66}{0.27\times 0.82}\\\\K_p=3.52$

Now, calculating the value of $\Delta G$ by using equation 1:

R = Gas constant = $8.314J/K mol$

T = temperature = 2000 K

$K_p$ = equilibrium constant in terms of partial pressure = 3.52

Putting values in equation 1, we get:

$\Delta G=-(8.314J/Kmol)\times 2000K\times \ln (3.52)\\\\\Delta G=-20925.68J/mol$

Converting this into kilo joules, we use the conversion factor:

1 kJ = 1000 J

So, -20925.68 J/mol = -20.925 kJ/mol

Hence, the value of $\Delta G$ for the chemical equation is -20.925 kJ/mol