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2 answers:
Answer: Option (a) is the correct answer.
Explanation:
Rate of a reaction gets affected by change in temperature as when we decrease the temperature then reactant molecules lose kinetic energy. As a result, there occurs decrease in number of collisions between the molecules.
Hence, rate of reaction also decreases with decrease in temperature.
Whereas when we increase the concentration from 30 mg to 60 mg then there is increase in number of reactant molecules. Therefore, there will be increase in number of collisions between the molecules.
Also, when substance is placed in smaller container then molecules come closer to each other and thus collide more frequently. So, rate of reaction will also increase.
On the other hand, grinding the substance into a powder will also increase the number of reactant particles. Thus, this will also increase the rate of reaction.
Thus, we can conclude that changing the temperature from to
will decrease the rate of a reaction.
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Answer:
a.
b. 146.0 g
Explanation:
Question 1 (a). Just as the problem states, liquid nitroglycerin decomposes into nitrogen gas , oxygen gas
, water vapor
and carbon dioxide
. Let's write the decomposition of nitroglycerin into these 4 components:
Now we need to balance the equation. Firstly, notice we have 3 carbon atoms on the left and 1 on the right, so let's multiply carbon dioxide by 3:
Now, we have 3 nitrogen atoms on the left and 2 on the right, so let's multiply nitrogen on the right by :
We have 5 hydrogen atoms on the left, 2 on the right, so let's multiply the right-hand side by :
Finally, count the oxygen atoms. We have a total of 9 on the left. On the right we have (excluding oxygen molecule):
This leaves of oxygen. Since oxygen is diatomic, we need to take one fourth of it to get one half in total:
To make it look neater without fractional coefficients, multiply both sides by 4:
Question 2 (b). Now we can make use of the balanced chemical equation and apply it for the context of this separate problem. We're given the following variables:
Firstly, we may find moles of carbon dioxide produced using the ideal gas law .
Rearranging for moles, that is, dividing both sides by RT (here R is the ideal gas law constant):
According to the stoichiometry of the balanced chemical equation:
4 moles of nitroglycerin (ng) produce 12 moles of carbon dioxide. From here we can find moles o nitroglycerin knowing that:
Multiplying the number of moles of nitroglycerin by its molar mass will yield the mass of nitroglycerin decomposed: