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3 years ago

Which of the following is a synthesis reaction?

Chemistry

2 answers:

Anvisha [2.4K]3 years ago

8 0

Answer:

The correct answer is CO2 + H2O yields H2CO3

Explanation:

Hi!

Let's solve this!

Synthesis reactions are those that two compounds or elements come together to form another.

Let's analyze each of the reactions:

C2H4 + 3 O2 yields 2 CO2 + 2 H2O in this reaction there is a recombination of elements

2HBr yields H2 + Br2 in this reaction the hydrogen bromide is broken and two simpler molecules are formed

CO2 + H2O yields H2CO3 in this reaction two compounds come together and form one

F2 + 2 HCl yields Cl2 + 2 HF in this reaction there is a rearrangement of elements

After the analysis, we conclude that the correct answer is CO2 + H2O yields H2CO3

nadezda [96]3 years ago

6 0

Synthesis reaction is a reaction where two or more substances combine to form a new compound. <span>It is a reaction which releases energy in the form of heat and light. Therefore, it is an exothermic reaction. </span>From its the definition the correct answer is the third option where carbon dioxide and water combine to form carbonic acid.

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Given the equation C3H8(g) + O2(g) = CO2(g) + H2O(g) and that the enthalpies of formation for H2O(g) = -241.8 kJ/mol, CO2(g) = -

kari74 [83]

Answer: 72.4 kJ/mol

Explanation:

The balanced chemical reaction is,

$C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(l)$ $\Delta H=-2220.1kJ/mol$

The expression for enthalpy change is,

$\Delta H=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]$

$\Delta H=[(n_{CO_2}\times \Delta H_{CO_2})+(n_{H_2O}\times \Delta H_{H_2O})]-[(n_{O_2}\times \Delta H_{O_2})+(n_{C_3H_8}\times \Delta H_{C_3H_8})]$

where,

n = number of moles

$\Delta H_{O_2}=0$ (as heat of formation of substances in their standard state is zero

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

$-2220.1=[(3\times -393.5)+(4\times -241.8)]-[(5\times 0)+(1\times \Delta H_{C_3H_8})]$

$\Delta H_{C_3H_8}=72.4kJ/mol$

Therefore, the heat of formation of propane is 72.4 kJ/mol

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3 years ago

Calculate the vapor pressure at 25 ?c of hexane above the solution. the vapor pressure of pure hexane at 25 ?c is 151 torr.

Studentka2010 [4]

One of the many ways in order to solve for the vapor pressure of pure components at a given temperature is through the Antoine's equation which is written below,
P = 10^(A - B/C+T)
where A, B, and C are constants and T is the temperature in °C and P is the vapor pressure in mm Hg.
For hexane,
A = 7.01
B = 1246.33
C = 232.988

Substituting the known values,
P = 10^(7.01 - 1246.33/232.988+25)
<em> P = 151.199 mm Hg</em>

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4 years ago