It is a covalent bond because both carbon and oxygen are nonmetals. The formula will be CO² because the electrons between the atoms are being shared equally.

8 0

2 years ago

Read 2 more answers

Standard notation for 31,254,000

bearhunter [10]

That seems to be standard notation

4 0

3 years ago

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 355 K. Predict wheth

Elena-2011 [213]

Answer:

$\Delta S_{surr} = + 0.32113\: kJ/K$

Explanation:

Given: Entropy of surrounding: ΔSsurr = ?

Temperature: T= 355 K

The change in enthalpy of reaction: ΔH = -114 kJ

Pressure: P = constant

As we know, ΔH = -114 kJ ⇒ negative

Therefore, the given reaction is an exothermic reaction

Therefore, Entropy of surrounding at constant pressure is given by,

$\Delta S_{surr} = \frac{-\Delta H}{T}$

$\therefore \Delta S_{surr} = -\left (\frac{-114 kJ}{355 K} \right ) = + 0.32113\: kJ/K > 0$

In the given reaction:

2NO(g) + O₂(g) → 2NO₂(g)

As, the number of moles of gaseous products is less than the number of moles of gaseous reactants.

$\therefore \Delta S_{system} < 0$

As we know, for a spontaneous process, that the total entropy should be positive.

$\Delta S_{total} = \Delta S_{surr} + \Delta S_{system} > 0$

Therefore, at the given temperature,

if $\Delta S_{surr} > \Delta S_{system} \Rightarrow \Delta S_{total} > 0$ then the given reaction is spontaneous

if $\Delta S_{surr} < \Delta S_{system} \Rightarrow \Delta S_{total} < 0$ then the given reaction is non-spontaneous

6 0

3 years ago