Answer:
Option-A (<span> It would increase from bottom left to top right) is the correct answer.
Explanation:
As we know converting solids into liquids and converting liquids into gases require energy. This energy provided increases the energy of the state and its particles start moving with higher velocities. Therefore, the energy of solids will be lower than liquids and gases respectively. While, liquids have greater energy than solids but less energy than gases. And, gases are the most energetic than solids and liquids.</span>
Answer:
The answers to your questions are given below below
Explanation:
1. The calculation will require multiple steps because the unit of measurement of the theoretical and actual yield is different.
2. Determination of the percentage yield.
We'll begin by converting 6733 mg to g. This can be obtained as follow:
1000 mg = 1 g
Therefore,
6733 mg = 6733 mg × 1 g / 1000 mg
6733 mg = 6.733 g
Finally, we shall determine the percentage yield. This can be obtained as follow:
Theoretical yield = 14.79 g
Actual yield = 6.733 g
Percentage yield =?
Percentage yield = Actual yield /Theoretical yield × 100
Percentage yield = 6.733 / 14.79 × 100
Percentage yield = 673.3 / 14.79
Percentage yield = 45.5%
<u>Answer:</u> The enthalpy of the reaction is coming out to be 2231 kJ.
<u>Explanation:</u>
Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as 
The equation used to calculate enthalpy change is of a reaction is:
![\Delta H^o_{rxn}=\sum [n\times \Delta H^o_{(product)}]-\sum [n\times \Delta H^o_{(reactant)}]](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5Csum%20%5Bn%5Ctimes%20%5CDelta%20H%5Eo_%7B%28product%29%7D%5D-%5Csum%20%5Bn%5Ctimes%20%5CDelta%20H%5Eo_%7B%28reactant%29%7D%5D)
For the given chemical reaction:
The equation for the enthalpy change of the above reaction is:
![\Delta H^o_{rxn}=[(1\times \Delta H^o_{(C_4H_8(g))})]-[(1\times \Delta H^o_{(C_4H_4(g))})+(2\times \Delta H^o_{(H_2(g))})]](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B%281%5Ctimes%20%5CDelta%20H%5Eo_%7B%28C_4H_8%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20H%5Eo_%7B%28C_4H_4%28g%29%29%7D%29%2B%282%5Ctimes%20%5CDelta%20H%5Eo_%7B%28H_2%28g%29%29%7D%29%5D)
We are given:
Putting values in above equation, we get:
![\Delta H^o_{rxn}=[(1\times (-2755))]-[(1\times (-286))+(2\times (-2341))]\\\\\Delta H^o_{rxn}=2213kJ](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B%281%5Ctimes%20%28-2755%29%29%5D-%5B%281%5Ctimes%20%28-286%29%29%2B%282%5Ctimes%20%28-2341%29%29%5D%5C%5C%5C%5C%5CDelta%20H%5Eo_%7Brxn%7D%3D2213kJ)
Hence, the enthalpy of the reaction is coming out to be 2231 kJ.
According to the FDA, products labeled gluten-free must contain less than 20 milligrams of gluten
B. Apparently it's bitter. Did not know that
