Which equation is an example of a synthesis reaction

As NaOH is added to an aqueous solution, the pH will 1. decrease. 2. Not enough information is given to solve the problem. 3. be

Dominik [7]

PH increases when you add NaOH because it’s a strong base.

4 0

2 years ago

A sample of neon occupies a volume of 478 mL at STP. What will be the volume of the neon when the pressure is reduced to 93.3 kP

Andre45 [30]

The volume of neon when the pressure is reduced to 93.3 kPa is 519 mL.

Explanation:

The kinetic theory of gases is mostly based on Boyle's law. From the Boyle's law, the pressure experienced by any gas molecules is inversely proportional to volume of the gas molecules. Also this inverse relation is obeyed if and only if the number of moles and temperature of the gas molecules remained constant.

So, $P=\frac{1}{V}$

So if there is a change in pressure then there will be inverse change in volume. That means if there is decrease in the pressure of gas molecules then there will be increase in the volume and vice versa.

So the Boyle's law is combined as $P_{1} V_{1} = P_{2} V_{2}$

As here the initial pressure or $P_{1}$ is 1 atm or 101.3 kPa and the initial volume is 478 mL. Similarly, the final pressure is 93.3 kPa and the final volume will be

$101.3*10^{3}*478*10^{-3} = 93.3*10^{3} * V_{2}$

$V_{2} = 519 mL$

So, the volume of neon when the pressure is reduced to 93.3 kPa is 519 mL.

5 0

3 years ago

Initially, the chalk had a mass of 323.5 grams but upon completion, its mass had dropped to 301.2 grams. What is the change in m

11Alexandr11 [23.1K]

The changes the masses of chalk on the scale because when it was dropped in Golden Hammer

7 0

3 years ago

NaClO3 > NaCl + O2 <br> Balance

tiny-mole [99]

Answer:

Balancing Strategies: To balance this reaction it is best to get the Oxygen atoms on the reactant side of the equation to an even number. Once this is done everything else falls into place. Put a "2" in front of the NaClO3. Change the coefficient in front of the O2.

6 0

2 years ago

Which of the following must be true about a reaction if it is only spontaneous at high temperatures?

Anastaziya [24]

1) Answer is: It is endothermic, with both positive enthalpy and entropy changes.

Endothermic reactions (ΔH>0) that increase the entropy of the system (ΔS>0) are spontaneous at high temperatures.

The change in Gibbs free energy (ΔG), at constant temperature and pressure, is: ΔG=ΔH−TΔS.

ΔH is the change in enthalpy.

ΔS is change in entropy.

T is temperature of the system.

When ΔG is negative, a reaction (occurs without the addition of external energy) will be spontaneous (exergonic).

2) Answer is: It is endothermic and heat is added to the system.

There are two types of reaction:

1) endothermic reaction (chemical reaction that absorbs more energy than it releases, ΔH>0).

2) exothermic reaction (chemical reaction that releases more energy than it absorbs).

For example, the breakdown of ozone is an endothermic process. Ozone has lower energy than molecular oxygen (O₂) and oxygen atom, so ozone need energy to break bond between oxygen atoms.

3) Answer is: For every two AB produced, the reaction requires three A.

Balanced chemical reaction: 3A + B → 2AB.

From balanced chemical reaction: n(A) : n(AB) = 3 : 2.

n(A) = 3 · n(AB) ÷ 2.

A and B are reactants and AB is product of balanced chemical reaction.

For every two AB produced, the reaction requires one B.

4) Answer is:

the amount of required activation energy = potential energy of the B - potential energy of the reactants A.

the enthalpy change of the reaction = potential energy of the products C - potential energy of the reactants A.

For all chemical reaction some energy is required and that energy is called activation energy (energy that needs to be absorbed for a chemical reaction to start).

This is endothermic reaction.

3 0

3 years ago