All categories

3 years ago

The formula for aluminum fluoride is electrically neutral which of the following is the correct

Chemistry

1 answer:

timama [110]3 years ago

8 0

AIF3

Hope this helps, God bless and have a good day.

You might be interested in

**ASAP**

jek_recluse [69]

the answer is C) . I hope this was helpful!

4 0

3 years ago

Read 2 more answers

How many moles at of a gas will occupy 2.5 L at STP?

Eduardwww [97]

Answer/Explanation

am not sure but I think its

Standard temperature = 273K

2.50 LTemperature

5 0

3 years ago

**ASAP PLEASE**

Anna007 [38]

The answer to your question is C.)

8 0

3 years ago

Read 2 more answers

For the reaction C2H4(g) + H2O(g) --> CH3CH2OH(g)

Dominik [7]

Answer : The value of equilibrium constant for this reaction at 262.0 K is $3.35\times 10^{2}$

Explanation :

As we know that,

$\Delta G^o=\Delta H^o-T\Delta S^o$

where,

$\Delta G^o$ = standard Gibbs free energy = ?

$\Delta H^o$ = standard enthalpy = -45.6 kJ = -45600 J

$\Delta S^o$ = standard entropy = -125.7 J/K

T = temperature of reaction = 262.0 K

Now put all the given values in the above formula, we get:

$\Delta G^o=(-45600J)-(262.0K\times -125.7J/K)$

$\Delta G^o=-12666.6J=-12.7kJ$

The relation between the equilibrium constant and standard Gibbs free energy is:

$\Delta G^o=-RT\times \ln k$

where,

$\Delta G^o$ = standard Gibbs free energy = -12666.6 J

R = gas constant = 8.314 J/K.mol

T = temperature = 262.0 K

K = equilibrium constant = ?

Now put all the given values in the above formula, we get:

$-12666.6J=-(8.314J/K.mol)\times (262.0K)\times \ln k$

$k=3.35\times 10^{2}$

Therefore, the value of equilibrium constant for this reaction at 262.0 K is $3.35\times 10^{2}$

3 0

3 years ago

Which is an example of potential energy?

Setler79 [48]

Probably C hope this helps

5 0

2 years ago

Read 2 more answers