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Volgvan
3 years ago
8

What is the difference between the energy of spring A, stretched 0.6 meters, and spring B, stretched 0.3 meters, if they have th

e same spring constant? A. Spring A has more potential energy than spring B. B. Spring A has less potential energy than spring B. C. Springs A and B have the same potential energy. D. Springs A and B have the same kinetic energy.
Chemistry
1 answer:
Svetach [21]3 years ago
8 0

Your answer would be A, Spring A has more potential energy.

Potential energy is exactly what it sounds like - energy that has the potential to exist due to stressors, but doesn't yet. In this case, the spring is ready to jump back into its original position however it can't because of it still being stretched, therefore this tension is what creates potential energy.

When you measure potential energy, the one with greater of it is the one where it has more stress being placed on it. In this case, spring A is being stretched furthest so it has the most potential energy.

Hope this helped!

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A certain reaction is exothermic in the forward direction. The reaction has more moles of gas on the product side. Which of the
alexgriva [62]

Answer:

Decreasing the pressure

6 0
4 years ago
At 500 K the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) has Kp = 51 In an equilibrium mixture at 500 K, the partial pressure of NO is
Aleks [24]

Answer:

p3=0.36atm (partial pressure of NOCl)

Explanation:

2 NO(g) + Cl2(g) ⇌ 2 NOCl(g)  Kp = 51

lets assume the partial pressure of NO,Cl2 , and NOCl at eequilibrium are P1 , P2,and P3 respectively

Kp=\frac{[NOCl]^{2} }{[NO]^{2} [Cl_2] }

Kp=\frac{[p3]^{2} }{[p1]^{2} [p2] }

p1=0.125atm;

p2=0.165atm;

p3=?

Kp=51;

On solving;

p3=0.36atm (partial pressure of NOCl)

7 0
3 years ago
What intermolecular forces can occur between a CO3<br> ion and H2O molecules? List them
Orlov [11]

Answer:

The intermolecular forces between CO3^2- and H2O molecules are;

1) London dispersion forces

2) ion-dipole interaction

3) hydrogen bonding

Explanation:

Intermolecular forces are forces of attraction that exits between molecules. These forces are weaker in comparison to the intramolecular forces, such as the covalent or ionic bonds between atoms in a molecule.

Considering CO3^2- and H2O, we must remember that hydrogen bonds occur whenever hydrogen is bonded to a highly electronegative atom such as oxygen. The carbonate ion is a hydrogen bond acceptor.

Also, the London dispersion forces are present in all molecules and is the first intermolecular interaction in molecular substance. Lastly, ion-dipole interactions exists between water and the carbonate ion.

5 0
3 years ago
When calculating the equilibrium constant, aqueous solutes must be expressed in moles per liter (M), and gases must be expressed
alukav5142 [94]

Answer:

B. They are dimensionless ratios of the actual concentration or pressure divided by standard state concentration, which is 1 M for solutions and 1 bar for gases.

Explanation:

Activity of a substance is defined as the ratio of an effective concentration or an effective pressure to a standard state pressure or a standard state pressure. It is usually a unit less ratio.

Concentrations in an equilibrium constant are really dimensionless ratios of actual concentrations divided by standard state concentrations. Since standard states are 1 M for solutes, 1 bar for gases, and pure substances for solids and liquids, these are the units to be used.

Hence, activity is a fudge factor to ideal solutions that correct the true concentration. Activity of a gas and solute concentration is a ratio with no unit.

3 0
3 years ago
A mixture of hydrochloric and sulfuric acids is prepared so that it contains 0.315 M HCl and 0.125 M H2SO4. What volume of 0.55
Xelga [282]

<u>Answer:</u> The volume of NaOH required is 402.9 mL

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}     .....(1)

  • <u>For HCl:</u>

Molarity of HCl solution = 0.315 M

Volume of solution = 503.4 mL = 0.5034 L   (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

0.315M=\frac{\text{Moles of HCl}}{0.5034L}\\\\\text{Moles of HCl}=(0.315mol/L\times 0.5034L)=0.1586mol

  • <u>For sulfuric acid:</u>

Molarity of sulfuric acid solution = 0.125 M

Volume of solution = 503.4 mL = 0.5034 L

Putting values in equation 1, we get:

0.125M=\frac{\text{Moles of }H_2SO_4}{0.5034L}\\\\\text{Moles of }H_2SO_4=(0.125mol/L\times 0.5034L)=0.0630mol

As, all of the acid is neutralized, so moles of NaOH = [0.1586 + 0.0630] moles = 0.2216 moles

Molarity of NaOH solution = 0.55 M

Moles of NaOH = 0.2216 moles

Putting values in equation 1, we get:

0.55M=\frac{0.2216}{\text{Volume of solution}}\\\\\text{Volume of solution}=\frac{0.2216}{0.55}=0.4029L=402.9mL

Hence, the volume of NaOH required is 402.9 mL

6 0
3 years ago
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