CHEMISTRY HIGH SCHOOL

Given the reaction below, which is the oxidized substance?
Mg + Cl2 Mg2+ + 2Clmc005-2

Answers

Answer 1
Answer:

Answer:

Mg+Cl2 = Mg2+2Cl

Explanation:

Firstly balance the equation

2Mg+Cl2=Mg2+2Cl

the oxidized substance=Cl2

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A solution of KCIO3 is prepared using 75 grams of the solute in enough water to make 0.250 liters of solution. The gram-formula mass of KCIO3 is 122 grams per mole.-- Determine the percent by mass of solute in the solution.

Dinitrogen trisulfide symbol

Answers

Dinitrogen trisulfide symbol:N2S3

Final answer:

The symbol for the compound dinitrogen trisulfide is N2S3. It is derived from the number of nitrogen and sulfur atoms present in the compound.

Explanation:

The chemical compound dinitrogen trisulfide is composed of two elements: nitrogen (N) and sulfur (S). When we name the compound according to IUPAC nomenclature rules, we consider the number of each type of atom present. Dinitrogen means there are two nitrogen atoms, represented by the subscript 2, and trisulfide implies that there are three sulfur atoms, signified by the subscript 3. Hence, the symbol or chemical formula for dinitrogen trisulfide is N2S3.

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Assuming constant pressure and temperature, how many moles of gas have been added to the initial 3 moles of gas when the volume increases from 2.0 to 4.0 liters?1.5 moles

2 moles

3 moles

6 moles

Answers

Answer:

Moles of gas added = 3 moles

Explanation:

Given:

Initial volume of gas, V1 = 2.0 L

Initial moles of gas, n1 = 3 moles

Final volume, V2 = 4.0 L

To determine:

The moles of gas added to bring the final volume to 4.0 L

Explanation:

Based on the ideal gas equation

PV = nRT

where P = pressure, V = volume ; n = moles of gas

R = gas constant, T = temperature

At constant P and T, the above equation becomes:

V/n = constant

This is the Avogadro's law

Therefore:

(V1)/(n1) = (V2)/(n2) \n\nn2 = (V2)/(V1) * n1 = (4.0 L)/(2.0L) * 3 = 6 moles

The final number of moles of gas = 6

Thus, moles added = Final - Initial = n2 - n1 = 6-3 = 3 moles
We first assume that the gas is ideal which is a safe assumption to approximate the answer to the problem. Then we need to know the ideal gas equation and that is:
 
PV=nRT 
where 
P- pressure
V- volume
n-number of moles-
R- ideal gas constant 
T-temperature. 

Since we know that P, T and V are constant, rearranging the equation would lead to:

P/TR = n/V or the ratio of the moles of gas and volume is constant. 

(3moles)/2L = (3+x)/4L 
where 
x is the additional moles. 

Solving for x = 3 moles. 

80.0 grams of NaOH is dissolved in water to make a 6.00 Lsolution. What is the molarity of the solution? (Molar mass of
NaOH = 40.0 g/mol) _M

Answers

The molarity of 6.00 liters of an aqueous solution that contains 80g of sodium hydroxide is 0.33M.

HOW TO CALCULATE MOLARITY:

  • The molarity of a solution can be calculated by dividing the number of moles by its volume. That is;

Molarity = no. of moles ÷ volume

  • According to this question, 6.0 liters of an aqueous solution that contains 80/40 = 2 mol of sodium hydroxide. The molarity is calculated as follows:

Molarity = 2mol ÷ 6L

Molarity = 0.33M

Therefore, the molarity of 2.0 liters of an aqueous solution that contains 0.50 mol of sodium hydroxide is 0.33M.

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What volume of oxygen gas is released at STP if 10.0 g of potassium chlorate is decomposed? (The molar mass of KClO3 is 122.55 g/mol.)

Answers

Given:

10g of potassium chlorate decomposed

STP

molar mass of KClO3 is 122.55 g/mol

 

Required:

Volume of oxygen gas

 

Solution:

The decomposition reaction is

2KClO3 → 2KCl + 3O2

                Moles of O2 = 10g KClO3 (1 mol KClO3/122.55 g/mol KClO3)(3 moles O2/2 moles KClO3) = 15 moles O2

                 Using ideal gas law: PV = nRT

               

                PV = nRT

                V = nRT/P

                V = (15 moles O2)(0.08206 L-atm/mol-K)(273K)/1 atm

                V = 336.04 L O2

                

Given the equation representing a reaction at equilibrium: N2(g) + 3H2(g) 2NH3(g) What occurs when the concentration of H2(g) is increased?

Answers

Given the equation representing a reaction at equilibrium: N2(g) + 3H2(g) = 2NH3(g). When the concentration of the hydrogen gas is increased, the equilibrium will tend to go to the products or to the forward reaction. Therefore, more products are formed.

Identify the atom oxidized, the atom reduced, the oxidizing agent, and the reducing agent. 2Fe + 3V2O3 -------> Fe2O3 + 6VO​

Answers

In the given reaction, Fe is the reducing agent and V is the oxidizing agent.

What is a reducing agent?

An atom or compound that loses its electrons to other substances in a reduction-oxidation reaction and gets oxidized to a higher valency state is called a reducing agent.

A reducing agent can be defined as one of the reactants of a redox reaction that reduces the other reactant by giving its electrons to the reactant. If the reducing agent can not give away its electrons to others in a reaction, then the reduction reaction cannot occur.

Given, the following chemical reaction:

2Fe + 3V₂O₃ → Fe₂O₃ + 6VO​

The V₂O₃ oxidation state of V:

2 x + 3(-2) = 0

2x = 6

x = + 3

The Fe₂O₃ oxidation state of Fe:

2 y + 3 (-2) = 0

2y = 6

y = + 3

The V acts as an oxidizing agent because it accepts one electron to change the oxidation state from +3 to +2.

Fe acts as a reducing agent because it gives out its electrons to change the oxidation state from 0 to +3.

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Explanation:

Fe- reducing agent (since it is oxidized to fe203)

v203- oxidizing agent(since it is reduced)
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