Answer: The results of Rutherford's gold foil experiment gave him the evidence to arrive at two conclusions: (1) an atom was much more than just empty space and scattered electrons and (2) an atom consists of a positive charge at the center where most of its mass is placed.
Explanation:
Ernest Rutherford performed an experiment in which he passed alpha particles through a thin gold foil sheet. Through this sheet some of the particles passed on to the other side but some of them were reflected back.
This experiment was done by Rutherford to prove than an atom contains a tiny and heavy nucleus. He concluded that an atom has more than empty space and electrons were present in scattered form.
Also, he concluded that an atom consists of a positive charge at the center where most of its mass is placed.
Thus, we can conclude that the results of Rutherford's gold foil experiment gave him the evidence to arrive at two conclusions: (1) an atom was much more than just empty space and scattered electrons and (2) an atom consists of a positive charge at the center where most of its mass is placed.
The fumaric acid reacts with water and forms fumarate anion and the hydronium ion which has acidic behavior. The reaction is reversible one due to the weakly hydrolysis of fumaric acid.
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Explanation:
↓↓↓↓↓↓↓
Density is the amount of mass in a given volume. It's a derived unit of measure. It is equal to mass divided by volume. It's measured in units such as grams per cubic centimeter and grams per milliliter. Density is the ratio of mass to volume. Density is a physical property of an object. It is degree of compactness of a substances. Relative density is used to separate solids, liquids, and gases. The gas in the container rises to the top because it has the least density. The liquids separate into individual layers based on their relative densities. The least dense liquid is on top. The most dense liquid is on bottom. The solids sink to the bottom of the container because they have the greatest density.
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B. The partial pressure of N2 is 101 kPa
<h3>Further explanation</h3>
Given
volume = 22.4 L
1.0 mol of nitrogen and 2.0 mol of hydrogen at 0°C
Required
Total pressure and partial pressure
Solution
Ideal gas law :
PV = nRT
n total = 3 mol
T = O °C + 273 = 273 K
P = nRT/V
P = 3 x 0.08205 x 273 / 22.4
P total = 3 atm = 303,975 kPa
P Nitrogen = 1/3 x 303.975 = 101.325 kPa
P Hydrogen = 2/3 x 303.975 = 202.65 kPa
Answer: The expression for equilibrium constant is ![\frac{[NH_3]^2}{[H_2]^3[N_2]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BNH_3%5D%5E2%7D%7B%5BH_2%5D%5E3%5BN_2%5D%7D)
Explanation: Equilibrium constant is the expression which relates the concentration of products and reactants preset at equilibrium at constant temperature. It is represented as 
For a general reaction:

The equilibrium constant is written as:
![k_c=\frac{[C]^c[D]^d}{[A]^a[B]^b}](https://tex.z-dn.net/?f=k_c%3D%5Cfrac%7B%5BC%5D%5Ec%5BD%5D%5Ed%7D%7B%5BA%5D%5Ea%5BB%5D%5Eb%7D)
Chemical reaction for the formation of ammonia is:


Expression for
is:
![k_c=\frac{[NH_3]^2}{[H_2]^3[N_2]}](https://tex.z-dn.net/?f=k_c%3D%5Cfrac%7B%5BNH_3%5D%5E2%7D%7B%5BH_2%5D%5E3%5BN_2%5D%7D)
![1.6\times 10^2=\frac{[NH_3]^2}{[H_2]^3[N_2]}](https://tex.z-dn.net/?f=1.6%5Ctimes%2010%5E2%3D%5Cfrac%7B%5BNH_3%5D%5E2%7D%7B%5BH_2%5D%5E3%5BN_2%5D%7D)