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3 years ago

Which type of chemical reaction occurs in C6H12 + 9O2 ----- 6CO2 + 6H2O?

Chemistry

1 answer:

Annette [7]3 years ago

4 0

Double replacement is happening

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Will calcium metal react with chromium (III) chloride? Explain your answer

iren [92.7K]

Calcium metal with chromium(III) chloride would react. Calcium metal is more reactive than chromium metal; therefore, putting calcium metal in chromium chloride would create a reaction, where as putting chromium metal in calcium chloride would not form any reaction.

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2 years ago

How many grams of NO can be made from 50 g of NH3? 4 NH3 + 5 O2 → 6 H2O + 4 NO

Evgen [1.6K]

0.08 because 4mol NO divided by 50g gives you your answer

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2 years ago

How many electrons does the oxygen atom need to become stable?

NemiM [27]

Answer:

2 electrons

Explanation:

Oxygen has 6 valence electrons and to be stable it needs 8. That means it needs 2 more electrons to have a full octet.

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2 years ago

Read 2 more answers

Calculate the standard enthalpy change for the reaction at 25 ∘ 25 ∘ C. Standard enthalpy of formation values can be found in th

WINSTONCH [101]

Answer: The standard enthalpy change of the reaction is coming out to be -16.3 kJ

Explanation:

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 $\Delta H$

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

$\Delta H_{rxn}=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]$

For the given chemical reaction:

$Mg(OH)_2(s)+2HCl(g)\rightarrow MgCl_2(s)+2H_2O(g)$

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

$\Delta H_{rxn}=[(1\times \Delta H_f_{(MgCl_2(s))})+(2\times \Delta H_f_{(H_2O(g))})]-[(1\times \Delta H_f_{(Mg(OH)_2(s))})+(2\times \Delta H_f_{(HCl(g))})]$

We are given:

$\Delta H_f_{(Mg(OH)_2(s))}=-924.5kJ/mol\\\Delta H_f_{(HCl(g))}=-92.30kJ/mol\\\Delta H_f_{(MgCl_2(s))}=-641.8kJ/mol\\\Delta H_f_{(H_2O(g))}=-241.8kJ/mol$

Putting values in above equation, we get:

$\Delta H_{rxn}=[(1\times (-641.8))+(2\times (-241.8))]-[(1\times (-924.5))+(2\times (-92.30))]\\\\\Delta H_{rxn}=-16.3kJ$

Hence, the standard enthalpy change of the reaction is coming out to be -16.3 kJ

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3 years ago

An object that sticks to iron

Dvinal [7]

Answer:

A magnet

Explanation:

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1 year ago