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3 years ago

Classify the four reactions that your group analyzed today as being either endothermic or exothermic

1 answer:

4 0

Chemical reactions are basically divided into two major classes depending on whether the reaction lose energy or gain energy from the environment during the course of the reaction. The two classes of reaction are exothermic and endothermic reaction.
An exothermic reaction is a type of reaction in which the reaction system lose energy to the environment and thus, the energy content of the reactants is more than that of the product formed. Because of this, the enthapyl change of an exothermic reaction is always negative.
An endothermic reaction is a type of reaction in which the reaction system absorb energy from the environment. Thus, the energy contents of the products is always higher than that of the reactants and the enthapyl change of the reaction is always positive. During the course of the reaction, the reaction container is usually cold to the touch because energy is been absorbed from the environment.

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Double replacement for Cu(NO3)2+Na2SO4

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Question 14 Ammonia and oxygen react to form nitrogen monoxide and water, like this: (g)(g)(g)(g) Write the pressure equilibrium

S_A_V [24]

Answer:

$Kp = \frac{(pNO)^4*p(H_2O)^6}{(pNH_3)^4*(pO_2)^5}$

Explanation:

The reaction is:

4NH₃(g) + 5O₂(g) ⇄ 4NO(g) + 6H₂O(g)

The equilibrium is achieved when the velocity of the formation of the products is equal to the velocity of the formation of the reactants, and then the concentrations and the partial pressures remain constant.

The equilibrium can be characterized by the equilibrium constant, which is a factor of the activity of each component. The solids and pure liquids have activity equal to 1, and so, they are not placed in the expression of the constant.

The other substances may have its activity substituted to the concentration, or the partial pressure (only gases). So, in the first case the constant will be the concentration equilibrium constant (Kc), and the second case the pressure equilibrium constant (Kp).

The constant is the ratio of the multiplication of the concentration (or pressure) of the products by the multiplication (or pressure) of the products. Each of the concentration (or pressure) is elevated by the coefficient of the substance.

So, for the reaction given:

$Kp = \frac{(pNO)^4*p(H_2O)^6}{(pNH_3)^4*(pO_2)^5}$

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3 years ago

How many moles of metallic aluminum (al) could be produced from al3+ at a current of 0.09 amperes for 964,853 seconds?

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Approximately 0.# moles, below is the solution to your problem.

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3 years ago

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A 1.362 g sample of an iron ore that contained Fe3O4 was dissolved in acid and all of the iron was reduced to Fe2+. The solution

tino4ka555 [31]

Based on the equation of the reaction;

the mass of iron (ii) ion present in the sample ore is 0.31 g
the percent mass of iron in the ore is 22.8%

<h3>What is the percentage mass of iron in the ore?</h3>

The percentage mass of iron in the ore is determined from the net ionic equation of the reaction as follows:

5 Fe²⁺ + MnO₄⁻ + 8H+ ---> 5 Fe³⁺ + Mn²⁺ + 4 H₂O

The mole ratio of the reaction shows that 5 moles of the iron (ii) ion is oxidized by 1 mole of tetraoxomanganate (vii) ion, MnO₄⁻.

The moles of tetraoxomanganate (vii) ion, MnO₄⁻ that reacted with al the iron present in the ore is determined as follows:

Moles of substance = molarity * volume in liters

Moles of tetraoxomanganate (vii) ion, MnO₄⁻ = 0.0281 * 39.42/1000

Moles of tetraoxomanganate (vii) ion, MnO₄⁻ = 0.001108 moles

Moles of iron (ii) ion present in the sample = 0.001108 * 5

Moles of iron (ii) ion present in the sample = 0.00554 moles

Mass of iron (ii) ion present in the sample = 0.00554 * 56

Mass of iron (ii) ion present in the sample = 0.31 g

Percent mass of iron in the ore = 0.31/1.362 * 100%

Percent mass of iron in the ore = 22.8%

Learn more about percentage mass at: brainly.com/question/26150306

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1 year ago