Answer:
Explanation:
1. Calculate the molar mass of N₂H₄
2N = 2 × 14 = 28
4H = 2 × 1 = <u> 4</u>
Tot. = 32
2. Calculate the mass percent of N
The answer is oxygen. (02)
Answer:
It is neutral (NR)
Explanation:
Salts are formed when the ionizable hydrogens in an acid is replaced by metallic or ammonium ions from bases. The reaction is known as a neutralization reaction.
The nature of a salt formed from this reaction depends on the nature of the reacting acid and base.
If the reaction is between a strong acid and strong base, the salt produced is a neutral salt.
If the reaction occurs between a strong acid and a weak base, the salt produced is acidic.
If the reaction occurs between a strong base and a weak acid, the salt produced is a basic salt.
Considering the salt above, LiNO3.
On hydrolysis, addition of water, the following products are obtained:
LiNO3 + H2O ----> LiOH + HNO3
The products obtained, LiOH and HNO3 are a strong base and a strong acid respectively. Therefore, the salt, LiNO3, is a neutral salt.
Answer:
She will observe that the pressure on the tire is higher.
Explanation:
By the ideal gas law, the pressure and the temperature are directly proportional, so, if the temperature increases the pressure increases too:
PV = nRT (P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature).
The temperature is a measure of the average kinetic energy of the gas molecules, so when the temperature increases, the energy also increases, and the gas molecules will move more quickly, so they will collide more often between themselves and in the wall. Those collisions will be with more force because the velocity is higher.
So, the pressure will be higher, because it is the result of collisions of the gas molecules with the walls of the tire.
Answer:
PNO₂ = 0.49 atm
PN₂O₄ = 0.45 atm
Explanation:
Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).
PV = nRT
n = m/M (m is the mass, and M the molar mass)
PxM = ρRT
ρ = PxM/RT
With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K
0.94Mavg = 63.9846
Mavg = 68.0687 g/mol
The molar mass of N is 14 g/mol and of O is 16 g/mol, than 
g/mol and 
g/mol. Calling y the molar fraction:
And,
So,
The partial pressure is the molar fraction multiplied by the total pressure so:
PNO₂ = 0.52x0.94 = 0.49 atm
PN₂O₄ = 0.48x0.94 = 0.45 atm
