Answer: +2
Explanation: Formula of oxide is MgO, because oxidation state of Mg in MgCO3 is +2.
Answer:
There are 29.4 grams of oxygen in the container
Explanation:
<u>Step 1: </u>Data given
Volume = 20.0 L
Pressure = 845 mmHg
Temperature = 22.0 °C
Molar mass of O2 = 32 g/mol
<u>Step 2:</u> Ideal gas law
p*V = n*R*T
⇒ p = the pressure of the gas = 845 mmHg = 1.11184
⇒ V = the volume of the gas = 20.0 L
⇒ n = the number of moles = TO BE DETERMINED
⇒R = the gasconstant = 0.08206 L*atm/K*mol
⇒ T = the temperature = 22°C + 273 = 295 Kelvin
n = (p*V)/(R*T)
n = (1.11184*20.0)/(0.08206*295)
n = 0.9186 moles
<u>Step 3:</u> Calculate mass of NO2
Mass of O2 = Moles O2 * Molar mass O2
Mass of O2 = 0.9186 moles * 32 g/mol
Mass of O2 = 29.4 grams
There are 29.4 grams of oxygen in the container
And the answer is equivalent to 0.64 moles of CO2.
It will help you
These values may represent the amount of pulling force that we exert on each other or in other words exert forces on both parties.
The answer may differ as well but keep in mind the values should be equal.
Note:
The answer is not about helping each other or the "spring balance". We are not talking about the literal moral values instead we are talking about Chemistry and Science.
Assuming we have 100 g of sample
30.45/MW of N 14g = 2.175
69.55/MW of O 16g = 4.34
4.34/2.185 = 2
for every 1 mole of N we have 2 moles of O
so the empirical formula would be NO2
without having the molecular weight of the entire molecule the molecular formula can not be determined with the information in your question
