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sertanlavr [38]
3 years ago
5

Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical

reaction:NOCL---> NO+CLUsing the thermodynamic information in the ALEKS&nRound your answer to zero decimal places
Chemistry
1 answer:
julia-pushkina [17]3 years ago
6 0

Answer:

43.0 kJ

Explanation:

The free energy (ΔG) measures the total energy that is presented in a thermodynamic system that is available to produce useful work, especially at thermal machines. In a reaction, the value of the variation of it indicates if the process is spontaneous or nonspontaneous because the free energy intends to decrease, so, if ΔG < 0, the reaction is spontaneous.

The standard value is measured at 25°C, 298 K, and the value of free energy varies with the temperature. It can be calculated by the standard-free energy of formation (G°f), and will be:

ΔG = ∑n*G°f products - ∑n*G°f reactants, where n is the coefficient of the substance in the balanced reaction.

By the balanced reaction given:

2NOCl(g) --> 2NO(g) + Cl2(g)

At ALEKS Data tab:

G°f, NOCl(g) = 66.1 kJ/mol

G°f, NO(g) = 87.6 kJ/mol

G°f, Cl2(g) = 0 kJ/mol

ΔG = 2*87.6 - 2*66.1

ΔG = 43.0 kJ

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Explanation:

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Calculate the molarity of the solution.
olga nikolaevna [1]

Answer:

ans. is 0.05

Explanation:

molarity=(mole of solute)/(litre of solution)

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Calculate the number of grams of Mg needed for this reaction to release enough energy to increase the temperature of 78 mL of wa
Vaselesa [24]

Answer:

We need 1.1 grams of Mg

Explanation:

Step 1: Data given

Volume of water = 78 mL

Initial temperature = 29 °C

Final temperature = 78 °C

The standard heats of formation

−285.8 kJ/mol H2O(l)

−924.54 kJ/mol Mg(OH)2(s)

Step 2: The equation

The heat is produced by the following reaction:

Mg(s)+2H2O(l)→Mg(OH)2(s)+H2(g)

Step 3: Calculate the mass of Mg needed

Using the standard heats of formation:

−285.8 kJ/mol H2O(l)

−924.54 kJ/mol Mg(OH)2(s)

Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g)

−924.54 kJ − (2 * −285.8 kJ) = −352.94 kJ/mol Mg

(4.184 J/g·°C) * (78 g) * (78 - 29)°C = 15991.248 J required

(15991.248 J) / (352940 J/mol Mg) * (24.3 g Mg/mol) = 1.1 g Mg

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7 0
3 years ago
A major component of gasoline is octane (C8H18). When liquid octane is burned in air it reacts with oxygen gas to produce carbon
Paraphin [41]

Answer:

The answer to your question is 0.4 moles of Oxygen

Explanation:

Data

Octane (C₈H₈)

Oxygen (O₂)

Carbon dioxide (CO₂)

Water (H₂O)

moles of water = ?

moles of Oxygen = 1

Balanced chemical reaction

                   C₈H₈  +10O₂  ⇒   8CO₂  +  4H₂O

              Reactant     Element     Products

                    8                 C                 8

                    8                 H                 8  

                   20                O               20  

Use proportions to solve this problem

                  10 moles of Oxygen ----------------- 4 moles of water

                    1 mol of Oxygen     ------------------ x

                    x = (4 x 1) / 10

                    x = 4 / 10

                    x = 0.4 moles of water

7 0
3 years ago
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