Podcast
Questions and Answers
how does concentration affect ROR?
how does concentration affect ROR?
increasing concentration of an aqueous reagent in a given volume increases ROR
more reactant particles in a given volume
=more frequent collisions
=more frequent successful collisions (colliding with enough energy to overcome activation energy and at the correct orientation)
=increase ROR
why will methane gas burn more quickly if under higher pressure
why will methane gas burn more quickly if under higher pressure
higher pressure means the molecules are pushed closer together, decreasing the distance between the molecules
decreasing the distance between the molecules increases the frequency of colisions between them
resulting in more frequent successful collisions (elaborate)
hence ROR increases
how does raising temperature of reagents increase ROR?
how does raising temperature of reagents increase ROR?
higher temperature = reactant particles have higher average kinetic energy
= increased proportion of collisions with energy that is equal to OR greater than Ea
= increased proportion of successful collisions
hence ROR increase
how does state of subdivision (surface area to volume ratio) affect ROR?
how does state of subdivision (surface area to volume ratio) affect ROR?
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state alteration that could increase reaction rate between solid copper oxide and sulfuric acid
state alteration that could increase reaction rate between solid copper oxide and sulfuric acid
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testing reaction CaCO3(s) + 2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g)
if a cotton wool plug is not used some solution may be lost due to its vigorous fizzing. How would the loss of solution cause an error in the determination for the mass of CO2(g) produced? Would this be a systematic or random error and how would it affect the calculated rate of reaction for each experiment? Explain.
testing reaction CaCO3(s) + 2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g)
if a cotton wool plug is not used some solution may be lost due to its vigorous fizzing. How would the loss of solution cause an error in the determination for the mass of CO2(g) produced? Would this be a systematic or random error and how would it affect the calculated rate of reaction for each experiment? Explain.
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the procedure the student used involved allowing the reaction mixture to lose 0.2g in mass, equivalent to an STP volume of CO2 of ~ 200mL, before she started timing for the 0.3g weight loss. Suggest a reason why it was important to do this. Remember carbon dioxide gas is much denser than air.
the procedure the student used involved allowing the reaction mixture to lose 0.2g in mass, equivalent to an STP volume of CO2 of ~ 200mL, before she started timing for the 0.3g weight loss. Suggest a reason why it was important to do this. Remember carbon dioxide gas is much denser than air.
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for reaction
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g), what are three ways to measure rate of reaction
for reaction Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g), what are three ways to measure rate of reaction
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