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A student runs an experiment to decompose hydrogen peroxide to produce oxygen and water. Increasing the temperature of hydrogen peroxide increases the rate of reaction. Explain why.

When the hydrogen peroxide is heated, the particles have more energy so move faster. This means that they will collide more often, increasing the likelihood of successful collisions. More successful collisio...
YA
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Calculate the pH of 0.1M Benzoic Acid (C6H5COOH). Ka = 6.3x10-5 M

Ka = [H + ][B - ]/[HB]Benzoic acid dissociates to C6H6COO - and H + - this is a 1:1 ratio so the concentrations are equal hence [H + ][B - ] = [H + ] 2 6.3x10-5 = [H + ] 2 /0.16.3x10-6 = [H + ] 2 therefore H...
MB
Answered by Michael B. • Chemistry tutor
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Explain the effect of increasing concentraion of O2 on the equilibrium position of this gas phase reaction and what you might see given that Nitrogen Oxide and Nitrogen Dioxide appear colourless and brown respectively. NO + 0.5O2 ----> NO2

Using "Le Chatelier's principle", the equilbrium will seek to oppose the change made to the reaction. In order to counter the increase in oxygen concentration, the reaction will shift to the right ...
AB
Answered by Amman B. • Chemistry tutor
4140 Views

Chlorine reacts with potassium bromide to form potassium chloride and bromine. In this reaction chlorine forms chloride ions: Cl2 + 2KBr --> 2KCl + Br2. Explain, using the equation, how you know that chlorine has been reduced.

It is reduced because it gains an electron in the reaction and reduction is the gain of electrons, therefore the chlorine has been reduced.
CB
Answered by Charles B. • Chemistry tutor
71290 Views

Define the term 'Bronsted-Lowry acid'

A proton ( H+ ion) donor
Answered by • Chemistry tutor
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