The force reduces
Explanation:
According to Coulomb's law, the force between the charges will reduce if the separation between the charges increases.
Coulomb's law states that "the force between two charges is a directly proportional to the product of the magnitude of the charges and inversely proportional to the square of their separation.".
F = ![\frac{K q_{1} q_{2} }{r^{2} }](https://tex.z-dn.net/?f=%5Cfrac%7BK%20q_%7B1%7D%20q_%7B2%7D%20%7D%7Br%5E%7B2%7D%20%7D)
where F is the electric field force
K is the constant of the field
is charge 1
is charge 2
r is the separation
We see that the separation is inversely proportional to the force between the charges. The larger the separation, the weaker or smaller the force.
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Answer: 1, 3, and 4
Explanation: i just did it
Answer: the answer is c.The unbalanced push causes the cart to speed up.
Explanation:
The application of an unbalanced force (the push) causes the cart to speed up. When the cart is in constant motion, the forces are balanced and there is no speeding up. Once an unbalanced force is added, the cart's speed changes.
2 or more simple machines I hope this help :)
Answer: The enthalpy of reaction is, -206.18 kJ
Explanation:-
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The final reaction is
![\Delta H_{rxn}=?](https://tex.z-dn.net/?f=%5CDelta%20H_%7Brxn%7D%3D%3F)
The intermediate balanced chemical reaction will be,
(1)
![\Delta H_1=-110.5kJ](https://tex.z-dn.net/?f=%5CDelta%20H_1%3D-110.5kJ)
(2)
![\Delta H_2=-74.85kJ](https://tex.z-dn.net/?f=%5CDelta%20H_2%3D-74.85kJ)
(3)
![\Delta H_3=-241.83kJ](https://tex.z-dn.net/?f=%5CDelta%20H_3%3D-241.83kJ)
Now adding (2) and (3) and subtracting (1) , we get :
![\Delta H_{rxn}=(\Delta H_2+\Delta H_3)-\Delta H_1](https://tex.z-dn.net/?f=%5CDelta%20H_%7Brxn%7D%3D%28%5CDelta%20H_2%2B%5CDelta%20H_3%29-%5CDelta%20H_1)
![\Delta H_{rxn}=((-74.85)+(-241.83))-(-110.5)](https://tex.z-dn.net/?f=%5CDelta%20H_%7Brxn%7D%3D%28%28-74.85%29%2B%28-241.83%29%29-%28-110.5%29)
![\Delta H_{rxn}=-206.18kJ](https://tex.z-dn.net/?f=%5CDelta%20H_%7Brxn%7D%3D-206.18kJ)
Therefore, the enthalpy of reaction is, -206.18 kJ