Answer:
- The last option: <u><em>Decrease the volume to increase pressure and to increase concentration.</em></u>
Explanation:
You can support your choice on basis of the collision theory.
According to the collision theory, the chemical reactions happen when the molecules collide with each other, in the correct orientation and with enough kinetic energy to overcome the activation energy.
As consequence, the larger the number of collisions the larger the rate of a reaction.
In the case of a reaction that involves gases, decreasing the volume, will increase the pressure and the concentration (volume is inversely related to both the pressure and the concentration) causing the molecules to be closer to each other and to collide with higher frequency, this is you will expect more collisions, and so an increase on the rate of the reaction. That is expressed by the last choice: decrease the volumen to increase pressure and to increase concentration.
Answer:
The attraction of the polar water molecules for other molecules
Explanation:
I think the answer is (4) 600.K and 0.50 atm, for gases behave most ideally at high temperature and low pressure.
Hope this helps~
Answer:
2040 kJ
Explanation:
Step 1: Calculate the energy provided by 21 g of protein
17 kJ are provided per gram of protein.
21 g × 17 kJ/g = 357 kJ
Step 2: Calculate the energy provided by 59 g of carbohydrate
17 kJ are provided per gram of carbohydrate.
59 g × 17 kJ/g = 1003 kJ
Step 3: Calculate the energy provided by 18 g of fat
38 kJ are provided per gram of fat.
18 g × 38 kJ/g = 684 kJ
Step 4: Calculate the total energy provided by the dinner
357 kJ + 1003 kJ + 684 kJ = 2044 kJ ≈ 2040 kJ
Answer:
Explanation:
Hello,
In this case, given the amounts of water and carbon dioxide we should invert the given reaction as hydrogen will be producted rather than consumed:
Consequently, the equilibrium constant is also inverted:
In such a way, we can now propose the law of mass action:
![Kc'=\frac{[H_2][CO_2]}{[H_2O][CO]}](https://tex.z-dn.net/?f=Kc%27%3D%5Cfrac%7B%5BH_2%5D%5BCO_2%5D%7D%7B%5BH_2O%5D%5BCO%5D%7D)
And we can express it in terms of the initial concentrations of the reactants and the change 
due to the reaction extent:
![Kc'=\frac{(x)(x)}{([H_2O]_0-x)([CO]_0-x)}=1.87](https://tex.z-dn.net/?f=Kc%27%3D%5Cfrac%7B%28x%29%28x%29%7D%7B%28%5BH_2O%5D_0-x%29%28%5BCO%5D_0-x%29%7D%3D1.87)
Thus, we compute the initial concentration which are same, since equal amount of moles are given:
![[H_2O]_0=[CO]_0=\frac{0.680mol}{70.0L}=0.0097M](https://tex.z-dn.net/?f=%5BH_2O%5D_0%3D%5BCO%5D_0%3D%5Cfrac%7B0.680mol%7D%7B70.0L%7D%3D0.0097M)
Hence, solving for by using the quardratic equation or solver, we obtain:
For which the correct value is 0.00561M since the other one will produce negative concentrations of water and carbon monoxide at equilibrium. Therefore, the number of moles of hydrogen at equilibrium for the same 70.0-L container turn out:
Best regards.
