Explanation:
there is 2 nitrogen but if you mean nitrate is 6
The relative mass of each element can be found from the periodic table (the larger number). For instance, P2O5, P = 31.0 O = 16.0, thus the formula mass (Mr) is 2(31) + 5(16) = 142 amu (atomic mass unit). I used a not really specific periodic table. Maybe your teacher is referring to open Schoology (a website where teacher can post files or announcements to students in his or her class). Sorry if i got something mistaken.
Answer:
1.Metals
These are very hard except sodium
These are malleable and ductile pieces
These are shiny
Electropositive in nature
Non-metals
These are soft except diamond
These are brittle and can break down into pieces
These are non-lustrous except iodine
Electronegative in nature
2. The electrochemical series helps to pick out substances that are good oxidizing agents and those which are good reducing agents.In an electrochemical series the species which are placed above hydrogen are more difficult to be reduced and their standard reduction potential values are negative.
3. Arrhenius theory, theory, introduced in 1887 by the Swedish scientist Svante Arrhenius, that acids are substances that dissociate in water to yield electrically charged atoms or molecules, called ions, one of which is a hydrogen ion (H+), and that bases ionize in water to yield hydroxide ions (OH−).
4. The common application of indicators is the detection of end points of titrations. The colour of an indicator alters when the acidity or the oxidizing strength of the solution, or the concentration of a certain chemical species, reaches a critical range of values.
The density is mass divided by volume
Answer:
Total pressure = 27.35 atm
Explanation:
Given data:
Mass of nitrogen = 12 g
Mass of H₂ = 0.40 mol
Mass of oxygen = 9.0 g
Volume of Container = 1 L
Temperature = 27 °C (27+273 = 300 K)
Total Pressure = ?
Solution:
First of all we will calculate the number of moles of individual gas.
Number of moles = mass/ molar mass
Number of moles = 12 g/ 28 g/mol
Number of moles = 0.43 mol
Pressure of N₂:
PV = nRT
P = nRT/V
P = 0.43 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 10.6 atm
Number of moles of Oxygen:
Number of moles = mass/ molar mass
Number of moles = 9 g/ 32 g/mol
Number of moles = 0.28 mol
Pressure of O₂:
PV = nRT
P = nRT/V
P = 0.28 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 6.9 atm
Pressure of H₂:
PV = nRT
P = nRT/V
P = 0.40 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 9.85 atm
Total pressure:
Total pressure = Pressure of H₂ + Pressure of O₂ + Pressure of N₂
Total pressure = 9.85 atm + 6.9 atm + 10.6 atm
Total pressure = 27.35 atm
