In the PhET Reactions & Rates (http://openstaxcollege.org/I/16PHETreaction) interactive, on the Many Collisions tab, set up a simulation with 15 molecules of A and 10 molecules of BC. Select “Show Bonds**#x201D; under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click “Pause" and then “Reset All,” and then enter 15 molecules of A and 10 molecules of BC once again. Select “Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
In the PhET Reactions & Rates (http://openstaxcollege.org/I/16PHETreaction) interactive, on the Many Collisions tab, set up a simulation with 15 molecules of A and 10 molecules of BC. Select “Show Bonds**#x201D; under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click “Pause" and then “Reset All,” and then enter 15 molecules of A and 10 molecules of BC once again. Select “Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
In the PhET Reactions & Rates (http://openstaxcollege.org/I/16PHETreaction) interactive, on the Many Collisions tab, set up a simulation with 15 molecules of A and 10 molecules of BC. Select “Show Bonds**#x201D; under Options.
(a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow?
(b) Click “Pause" and then “Reset All,” and then enter 15 molecules of A and 10 molecules of BC once again. Select “Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
"Water gas" is an industrial fuel composed of a mixture of carbon monoxide and hydrogen gases. When this
fuel is burned, carbon dioxide and water result. From the information given below, write a balanced equation
and determine the enthalpy of this reaction:
CO(g) + O2(g) → CO₂(g) + 282.8 kJ
H2(g) + O2(g) → H₂O(g) + 241.8 kJ
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4. Calculate AG for the following reaction at 25°C. Will the reaction occur (be spontaneous)? How do you
know?
NH3(g) + HCl(g) → NH4Cl(s)
AH=-176.0 kJ
AS-284.8 J-K-1
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