Answer : The balanced two-half reactions will be,
Oxidation half reaction : 
Reduction half reaction : 
Explanation :
Voltaic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy. It is also known as the galvanic cell or electrochemical cell.
In the voltaic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.
The given redox reaction is:
The balanced two-half reactions will be,
Oxidation half reaction :
Reduction half reaction :
Answer:
Explanation:
The reason for that is because atoms make elements needed for survival(oxygen, hydrogen, nitrogen, carbon, etc.).
Answer:
The boiling point of a liquid is the temperature at which its vapor pressure is equal to the pressure of the gas above it.The normal boiling point of a liquid is the temperature at which its vapor pressure is equal to one atmosphere (760 torr). Microscopic view inside a bubble in boiling water.
Explanation:
Answer:
1.03 grams of hydrogen is produced from 12.5 g of Mg reacting with hydrochloric acid.
Explanation:
The balanced reaction is:
Mg+ 2 HCl → MgCl₂ + H₂
By stoichiometry of the reaction, the following amounts of moles of each compound participate in the reaction:
- Mg: 1 mole
- HCl: 2 moles
- MgCl₂: 1 mole
- H₂: 1 mole
Being the molar mass of each compound:
- Mg: 24.31 g/mole
- HCl: 36.45 g/mole
- MgCl₂: 95.21 g/mole
- H₂: 2 g/mole
By reaction stoichiometry, the following mass amounts of each compound participate in the reaction:
- Mg: 1 mole* 24.31 g/mole= 24.31 g
- HCl: 2 moles* 36.45 g/mole= 72.9 g
- MgCl₂: 1 mole* 95.21 g/mole= 95.21 g
- H₂: 1 mole* 2 g/mole= 2 g
Then you can apply the following rule of three: if by stoichiometry 24.31 grams of Mg produces 2 grams of H₂, 12.5 grams of Mg produces how much mass of H₂?
mass of H₂= 1.03 grams
<u><em>1.03 grams of hydrogen is produced from 12.5 g of Mg reacting with hydrochloric acid.</em></u>
Answer:
The volume of the gas at 100°C is 4.6189 liters.
Explanation:
For this problem we are going to use Charles' law. Charles' law states that the volume is directly proportional to temperature given that the pressure is constant. In order to use the equation, the unit of temperature should be in Kelvin.
The working equation is:
=
where V1 and T1 are the initial volume and temperature while V2 and T2 are the final conditions.
Let us convert first the temperatures before solving for the final volume.
To convert Celsius to Kelvin just add 273.15 to temperature in Celsius.
50°C + 273.15 = 323.15 K
100°C + 273.15 = 373.15 K
Solving for the final volume:
V₂ =
V₂ =
V₂ = 4.6189 L
Therefore the final volume of the gas at 100°C is 4.6189 L.
Explanation:
