Propanol molecular formula is C₃H₇OH
the balanced reaction for combustion of propanol is as follows;
2C₃H₇OH + 9O₂ --> 6CO₂ + 8H₂O
Molar ratio of reactants to products can be found out by the stoichiometry.
By looking at the coefficients of reactants and products in the balanced reaction equation, molar ratio can determined.
Therefore the molar ratio of propanol to CO₂ is 2:6, simplified --> 1:3
the oxidation state of each atom
Answer:
The correct option is;
(B) 1 s², 2s², 2p⁶, 3s², 3p³
Explanation:
The electron configuration is the outline of the electron arrangement about a nucleus
In the systemic pattern of electron arrangement within an atom, there are, s, p, d, f orbitals
The maximum number of electrons in an s, p and d orbital = 2, 6, and 10 respectively
Based on Aufbau's principle the electrons are arranged based on the order of their energy level
The charge is presented by the number of electrons in the outermost shell, an element able to form an ion of charge of -3 will gain 3 electrons to complete its outermost shell
Among the options given, option B is the only option that has the capacity to take the electrons to complete the number of electrons in the p orbital outermost shell to 6 from 3, that is 3p³ + 3e⁻→ 3p⁶.
Answer:
A chemical reaction is the process in which atoms present in the starting substances rearrange to give new chemical combinations present in the substances formed by the reaction. These starting substances of a chemical reaction are called the reactants, and the new substances that result are called the products.
Answer:
20 moles
Explanation:
The important thing to realize here is that you're working under STP conditions, which implies that you can use the molar volume of a gas at STP to find how many moles of helium will occupy that volume.
Now, the molar volume of a gas represents the volume occupied by one mole of a gas under some specific conditions for pressure and temperature.
Starting from the ideal gas law equation
PV=nRT
you can say that the molar volume of gas at a pressure P and a temperature T will be equal to
Vn=RTP
Now, Standard Temperature and Pressureconditions are defined as a pressure of 100 kPaand a temperature of 0∘C. Under these specific conditions, the molar volume of a gas will be equal to
Vn=0.0821⋅atm⋅Lmol⋅K⋅(273.15+0)K100101.325atm
Vn=22.7 L/mol
This of course implies that one mole of any ideal gas will occupy 22.7 L.
In your case, the volume of the gas is said to be equal to 500 L. This means that you will have
500L⋅1 mole He22.7L=22.026 moles He
Rounded to one sig fig, the number of sig figs you have for the volume of the gas, the answer will be
nHe=20 moles
SIDE NOTE Many textbooks and online sources still list STP conditions as a pressure of 1 atmand a temperature of 0∘C.
Under these conditions for pressure and temperature, one mole of any ideal gas occupies 22.4 L. If these are the values for STP given to you by your instructor, make sure to redo the calculations using 22.4 L instead of 22.7 L
