What Are the Products and Balancing Steps for These Chemical Reactions?

AI Thread Summary
The discussion centers on two chemical reactions: the first involves the synthesis of an acid from chlorine monoxide and water, with the correct product identified as hypochlorous acid (HClO) rather than chloric acid (HClO3). The second reaction is a combustion of propane (C3H8) with oxygen, producing carbon dioxide (CO2) and water (H2O), with the balanced equation being C3H8 + 5O2 = 3CO2 + 4H2O. Participants clarify the nature of these reactions, emphasizing the importance of proper balancing and product identification. The conversation highlights common misconceptions and the need for accurate chemical knowledge. Understanding these reactions is essential for mastering basic chemistry concepts.
msimard8
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Here is my first question.

Cl2O + H2O ------->

I am pretty sure this is a synthesis reaction becasue it there is non metal oxide and a water. I also know a non metal oxide plus a water forms an acid. I predict this to be HClO3.

If that is the correct answer, I can't seem to balance the equation. Help


My second question is

C3H8 + 5O2 -----> ??

I am guessing this is single displacement. How to I obtain the product. Then how do i balance it.

Help
 
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I am not too sure on the first reaction, you don't normally see Chlorine with a positie charge like that.

Bu the second reaction is a simple combustion reaction, producing Carbon Dioxide and Water (Steam).
Propane and excess Oxygen combust completely to form Carbon Dioxide and Water,
C3H8 + 5 O2 = 3 CO2 + 4 H2O
All complete combustion reactions profuce CO2 and H2O.
 
first equation gives you 2 HClO (hypochlorous acid)
Found it on google
 
Thread 'Confusion regarding a chemical kinetics problem'
TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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