A #5 L# container holds #5 # mol and #10 # mol of gasses A and B, respectively. Every five of molecules of gas B bind to two molecule of gas A and the reaction changes the temperature from #320^oK# to #450 ^oK#. By how much does the pressure change?
There is a change of
First, we calculate the initial pressure using the Ideal Gas Law:
Here,
And input:
Now, we need the equation that took place. It is:
Here,
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To solve this problem, we first need to calculate the initial and final number of moles of gas A and B, using the ideal gas law. Then, we can determine the initial and final volumes of the gases at the given temperature. Finally, we can use the ideal gas law again to find the initial and final pressures, and then calculate the change in pressure.

Calculate initial moles of A and B: Initial moles of A = 5 mol Initial moles of B = 10 mol

Calculate final moles of A and B after the reaction: For every 5 molecules of B, 2 molecules of A react. So, after the reaction, the number of remaining molecules of B = 10 mol  (10 mol / 5) * 2 = 6 mol Remaining moles of A = 5 mol  (10 mol / 5) = 3 mol

Use the ideal gas law to find the initial and final volumes of the gases: Initial volume = 5 L Initial temperature = 320 K Final temperature = 450 K

Calculate the initial and final pressures using the ideal gas law: (P_1V_1 = n_1RT_1) and (P_2V_2 = n_2RT_2)

Calculate the change in pressure: (\Delta P = P_2  P_1)
By calculating the values using the given information and equations above, you can find the change in pressure.
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When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
 A #6 L# container holds #4 # mol and #6 # mol of gasses A and B, respectively. Groups of three of molecules of gas B bind to two molecules of gas A and the reaction changes the temperature from #480^oK# to #270^oK#. How much does the pressure change?
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