The rate of a reaction can be increased by:
-using a catalyst- it lowers the activation energy and leads to less energy required to break bonds of reactants. This lower activation energy leads to more products formed with less time, hence an increase reaction rate.
-increasing temperature- the particles of a molecule move faster and undergo more collision which leads to an increase in the speed of the reaction.
-increasing pressure- means there is more particles of reactants in a reduced volume. The particles do not need to move long distances to find another particle to react with, hence the rate of reaction increases.
Using an inhibitor will not increase the rate of the reaction because, an inhibitor binds to the active site where a catalyst is supposed to act. This means a higher activation energy and thus a decrease in reaction rate.
Likewise, decreasing the concentration implies few particles available to collide with each other and that slow down the speed of the reaction.
To
determine the percent ionization of the acid given, we make use of the acid
equilibrium constant (Ka) given. It is the ration of the equilibrium
concentrations of the dissociated ions and the acid. The dissociation reaction
of the HF acid would be as follows:<span>
HF = H+ + F-
The acid equilibrum constant would be expressed as follows:
Ka = [H+][F-] / [HF] = 3.5 x 10-4
To determine the equilibrium concentrations we use the ICE table,
HF
H+ F-
I 0.337 0
0
C -x +x
+x
---------------------------------------------
E 0.337-x x
x
3.5 x 10-4 = [H+][F-] / [HF]
3.5 x 10-4 = [x][x] / [0.337-x] </span>
Solving for x,
x = 0.01069 = [H+] = [F-]
percent ionization = 0.01069 / 0.337 x 100 = 3.17%
Answer:
pHe = 3.2 × 10⁻³ atm
pNe = 2.5 × 10⁻³ atm
P = 5.7 × 10⁻³ atm
Explanation:
Given data
Volume = 1.00 L
Temperature = 25°C + 273 = 298 K
mHe = 0.52 mg = 0.52 × 10⁻³ g
mNe = 2.05 mg = 2.05 × 10⁻³ g
The molar mass of He is 4.00 g/mol. The moles of He are:
0.52 × 10⁻³ g × (1 mol / 4.00 g) = 1.3 × 10⁻⁴ mol
We can find the partial pressure of He using the ideal gas equation.
P × V = n × R × T
P × 1.00 L = 1.3 × 10⁻⁴ mol × (0.082 atm.L/mol.K) × 298 K
P = 3.2 × 10⁻³ atm
The molar mass of Ne is 20.18 g/mol. The moles of Ne are:
2.05 × 10⁻³ g × (1 mol / 20.18 g) = 1.02 × 10⁻⁴ mol
We can find the partial pressure of Ne using the ideal gas equation.
P × V = n × R × T
P × 1.00 L = 1.02 × 10⁻⁴ mol × (0.082 atm.L/mol.K) × 298 K
P = 2.5 × 10⁻³ atm
The total pressure is the sum of the partial pressures.
P = 3.2 × 10⁻³ atm + 2.5 × 10⁻³ atm = 5.7 × 10⁻³ atm
Answer:Hope this helps!
Explanation:
You can use a flame test to help identify the composition of a sample. The test is used to identify metal ions (and certain other ions) based on the characteristic emission spectrum of the elements. The test is performed by dipping a wire or wooden splint into a sample solution or coating it with the powdered metal salt. The color of a gas flame is observed as the sample is heated. If a wooden splint is used, it's necessary to wave the sample through the flame to avoid setting the wood on fire. The color of the flame is compared against the flame colors known to be associated with the metals.
Each species is a separate type of organism.
- A species is a group of creatures that share similar traits. The same species of organisms are capable of sexual reproduction as well as interbreeding and producing fertile offspring. It is a fundamental unit of taxonomy and classification.
- The system is divided into seven categories: Kingdom, Phylum or Division, Class, Order, Family, Genus, and Species. Kingdom is the most inclusive category.
- In a group, many types of an organism can be included even if they do not share the same traits. But species is a group of organisms that share similar traits.
- For example, human beings are species as they are all alike in physical features, way of reproduction, etc. But the animal is considered a group because it included a variety of living beings.
Therefore, Each species is not considered a group.
Learn more about taxonomy here:
brainly.com/question/1304906
#SPJ9
