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4 years ago

Which of the aqueous solution does not conduct electricity ? 1.Ca(NO3)2 / 2.CH3NH2/ 3.CH3OH/ 4.CH3COOH

Chemistry

1 answer:

bezimeni [28]4 years ago

8 0

For an aqueous solution to conduct electricity, ions must be present in solution.

This means soluble salts will conduct electricity. Also, since acids and bases have ions in solution, they could also conduct electricity. Option 1 is a soluble salt. Options 2 and 4 are base and acid respectively. Option 3, though soluble in water, exist as a molecule, therefore its solution cannot conduct electricity.

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What element marks the boundary between using fusion and fission to release energy?

frez [133]

Answer:

matter

Explanation:

3 0

3 years ago

1. Consider the reaction: N2 (g) + O2 (g)  2NO (g) + Cl2 (g) A reaction mixture at 400 C has the following composition: [NO] =

Olegator [25]

Answer:

The reaction is not at the equilibrium, we have more products than reactants.

Explanation:

Step 1: Data given

Temperature = 400 °C

When Q=K, this means the system is at equilibrium. There will not be a shift to either the left or the right.

When Q<K,it means we have more reactants than products. The system will, as reaction, make more products, this will cause the equilibrium to move to the right.

When Q>K,it means we have more products than reactants. The system will, as reaction, make less products and more reactants, this will cause the equilibrium to move to the left.

[NO] = 0.01 M

[N2] = 0.001 M

[O2] = 0.001 M

Kc = 0.0156

Step 2: The balanced equation

N2 (g) + O2 (g) ⇆ 2NO (g) + Cl2 (g)

Step 3: Calculate Q

Q = [NO]²/[N2][O2]

Q = 0.01²/(0.01*0.001)

Q = 10

Q>>Kc

This means we have more products than reactants. The system will, as reaction, make less products and more reactants, this will cause the equilibrium to move to the left.

The reaction is not at the equilibrium, we have more products than reactants.

4 0

3 years ago

Which statement below correctly describes the relationship between Q and K for both reactions? Are these reactions spontaneous a

nikklg [1K]

Answer:

Q < K for both reactions. Both are spontaneous at those concentrations of substrate and product.

Explanation:

Hello,

In this case, the undergoing chemical reactions with their proper Gibbs free energy of reaction are:

$A->B;\Delta _rG^o=-13 kJ/mol$

$C ->D ;\Delta _rG^o=3.5 kJ/mol$

The cellular concentrations are as follows: [A] = 0.050 mM, [B] = 4.0 mM, [C] = 0.060 mM and [D] = 0.010 mM.

For each case, the reaction quotient is:

$Q_1=\frac{4.0mM}{0.050mM}=80\\ Q_2=\frac{0.010mM}{0.060mM}=0.167$

A typical temperature at a cell is about 30°C, in such a way, the equilibrium constants are:

$K_1=exp(-\frac{-13000J/mol}{8.314J/mol*K*303.15K} )=173.8\\K_2=exp(-\frac{3500J/mol}{8.314J/mol*K*303.15K} )=0.249$

Therefore, Q < K for both reactions. Both are spontaneous at those concentrations of substrate and product.

Best regards.

6 0

3 years ago

If ammonia is manufactured at 356 k, is the reaction spontaneous, given that the enthalpy and entropy change for the reaction ar

Alchen [17]

The reaction will be spontaneous if Gibb free energy is negative, according the following relation:
G = H - T*S
where G is Gibbs free energy, T is change of enthalpy , T is temperature and S is change of entropy
In the case of ammonia:
G = -93000 - 356*(-198) = -93000 + 70488 = -22512 j/mol
As G < 0 then the reaction is spontaneous.

5 0

4 years ago

What is the molarity of 50.84 g of Na2CO3 dissolved in 0.400 L solution?

borishaifa [10]

Answer:

1.20 M

Explanation:

Convert grams of Na₂CO₃ to moles. (50.84 g)/(105.99 g/mol) = 0.4797 mol

Molarity is (moles of solute)/(liters of solvent) = (0.4797 mol)/(0.400 L) = 1.20 M

4 0

3 years ago