All categories

3 years ago

All of the following are examples of matter except

Chemistry

1 answer:

Alexxandr [17]3 years ago

3 0

A. Heat because it does not take up space.

You might be interested in

A Bronsted-Lowry base is defined as a substance that

ICE Princess25 [194]

Answer:

Accepts Protons into it.

Explanation

7 0

3 years ago

Natural processes tend to increase the __________ of thermodynamic systems.

alekssr [168]

Answer:

the answer is c

Explanation:

6 0

3 years ago

Help please and thanks

Likurg_2 [28]

The first one is 2
The second is 1
The third is 6
And the fourth is 3

4 0

4 years ago

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.

algol13

Answer : The value of $\Delta G_{rxn}$ is -24.9 kJ/mol

Explanation :

First we have to calculate the value of 'Q'.

The given balanced chemical reaction is,

$Fe_2O_3(s)+3CO(g)\rightarrow 2Fe(s)+3CO_2(g)$

The expression for reaction quotient will be :

$Q=\frac{(p_{CO_2})^3}{(p_{CO})^3}$

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

Now put all the given values in this expression, we get

$Q=\frac{(2.1)^3}{(1.4)^2}$

$Q=3.375$

Now we have to calculate the value of $\Delta G_{rxn}$ .

The formula used for $\Delta G_{rxn}$ is:

$\Delta G_{rxn}=\Delta G^o+RT\ln Q$ ............(1)

where,

$\Delta G_{rxn}$ = Gibbs free energy for the reaction = ?

$\Delta G_^o$ = standard Gibbs free energy = -28.0 kJ/mol

R = gas constant = $8.314\times 10^{-3}kJ/mole.K$

T = temperature = 298 K

Q = reaction quotient = 3.375

Now put all the given values in the above formula 1, we get:

$\Delta G_{rxn}=(-28.0kJ/mol)+[(8.314\times 10^{-3}kJ/mole.K)\times (298K)\times \ln (3.375)$

$\Delta G_{rxn}=-24.9kJ/mol$

Therefore, the value of $\Delta G_{rxn}$ is -24.9 kJ/mol

5 0

3 years ago

Can anyone solve #2 or #3 i cannot figure them out

kompoz [17]

Answer:

sorry,,,,I can't

Explanation:

8 0

3 years ago