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3 years ago

In a exothermic reaction, is heat transfered to or from the surrounding

Chemistry

2 answers:

Anna71 [15]3 years ago

8 0

Heat is transferred to the surrounding. To remember this just think heat EXits to the surrounding

Monica [59]3 years ago

7 0

In an exothermic reaction, heat is transferred to the surrounding.

Hope this helps, have a great day ahead!

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A gas has a volume of 56.3L when its temperature is 280 K. What will volume be at 220K?

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lesantik [10]

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2 years ago

Read 2 more answers

Explain how changing the concentration The enthalpy change for the reaction, 3CO (g) 2Fe2O3 (s) Imported Asset Fe(s) 3CO2 (g), c

ycow [4]

<u>Answer:</u> For the given equation, only iron has the value of $\Delta H_f$ equal to 0 kJ.

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H^o$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f(product)]-\sum [n\times \Delta H^o_f(reactant)]$

For the given chemical reaction:

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

The equation for the enthalpy change of the above reaction is:

$\Delta H^o_{rxn}=[(1\times \Delta H^o_f_{(Fe(s))})+(3\times \Delta H^o_f_{(CO_2(g))})]-[(3\times \Delta H^o_f_{(CO(g))})+(2\times \Delta H^o_f_{(Fe_2O_3(s))})]$

The enthalpy of formation for the substances present in their elemental state is taken as 0.

Here, iron is present in its elemental state which is solid.

Hence, for the given equation, only iron has the value of $\Delta H_f$ equal to 0 kJ.

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2 years ago

Write a chemical equation for the reaction that occurs in the following cell: Cu|Cu2+(aq)||Ag+(aq)|Ag. Of the two metals, copper

KatRina [158]

Answer:

Answer is given below.

Explanation:

Anode is that electrode where oxidation occurs. Cathode is that electrode where reduction occurs.

In cell representation, half cell present left to salt-bridge notation $(\parallel )$ is anodic system and another half cell present right to salt-bridge notation $(\parallel )$ is cathodic system.

So anode is Cu and cathode is Ag.

oxidation: $Cu-2e^{-}\rightarrow Cu^{2+}(aq.)$

[reduction: $Ag^{+}+e^{-}\rightarrow Ag$ ] $\times 2$

-----------------------------------------------------------------------------------------------

chemical equation: $Cu+2Ag^{+}(aq.)\rightarrow Cu^{2+}(aq.)+2Ag$

Oxidizing agent is that species which takes electron from another species. Here $Ag^{+}(aq.)$ takes electron from Cu. Hence $Ag^{+}(aq.)$ is the oxidizing agent.

Reducing agent is that species which gives electron to another species. Here Cu gives electron to $Ag^{+}(aq.)$ . Hence Cu is the reducing agent.

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3 years ago