What is the relative molecular mass of the mixture of H2 and O2 with volume ratio a: B and mass ratio a: B What is the relative molecular mass of the mixture of H2 and O2 with volume ratio a: B and mass ratio a: B

What is the relative molecular mass of the mixture of H2 and O2 with volume ratio a: B and mass ratio a: B What is the relative molecular mass of the mixture of H2 and O2 with volume ratio a: B and mass ratio a: B

When the volume ratio is a: B, the mass ratio is a: B, the mass ratio is 1:16, and the average molecular weight is 17a / A + B
If the mass ratio is a: B, the mass ratio is 16A: B = volume ratio, the total volume is 16A + B. the average molecular weight is a + B / 16A + B

At the same temperature and pressure, the volume ratio of H2 and O2 with the same mass is 0

At the same temperature and pressure, the volume ratio of H2 and O2 with the same mass is (M / 2): (M / 32) = 16:1

At the same temperature and pressure, the same mass of O2, H2, N2, the volume of the three gases, the weight of the matter, the number of molecules

With the same mass, the smaller the relative molecular mass is, the greater the mass of matter is (n = m / M), so the mass of matter is H2 > N2 > O2. Under the same temperature and pressure, the volume of gas and the number of molecules are proportional to the mass of matter, so they are H2 > N2 > O2

Knowing the molar ratio, how to calculate the mass ratio?
The molar ratio of urea, furfuryl alcohol, formaldehyde and phenol is 1:0.92:2.59:0.28. What is their mass ratio? How to calculate?

Multiply the molar ratio by the corresponding molar mass of each substance
Molecular weight of urea 60
The molecular weight of furfuryl alcohol is 98
The molecular weight of formaldehyde is 30
The molecular weight of phenol is 84
The mass ratio of urea, furfuryl alcohol, formaldehyde and phenol is as follows:
1*60:0.92*98:2.59*30:0.28*84

What's the mole ratio mass
TEOS 1: NaOH (0.6) H2O (850) (mole ratio)
I want to know how to calculate the quality ratio. Can you teach me step by step

One mole of sodium hydroxide is 40 grams, one mole of water is 18 grams, so
m(NaOH):m(H2O)=40*0.6:18*850=24:15300
The unit is gram

The difference between atomic ratio and molar ratio?

Atomic ratio: the ratio of the number of different atoms
Mole ratio: the ratio of the amount of different substances

When the cube A and cube B are placed on the horizontal table, their pressure on the table is equal, and the ratio of pressure is 9:4, then the ratio of density of cube A and cube B is ()
A. 2：3B. 3：2C. 1：1D. 4：9

F1s1 = f2s2 ﹣ F1F2 = S1S2 = 94 ﹣ L1L2 = 32 ﹣ V1V2 = 278, F1F2 = m1m2 = 94 ﹣ ρ 1 ρ 2 = m1v1m2v2 = 92748 = 23

The problem of pressure when the temperature and density are the same in the container
When three sealed containers are filled with hydrogen, neon and oxygen, and their temperature and density are the same, the pressure of these three gases is arranged from small to large? Why

The order of pressure is: P oxygen < p neon < p hydrogen
The reasons are as follows:
According to the standard gas equation, PV = NRT
That is p = NRT / v
That is p = MRT / VM
That is p = ρ RT / m
∵ the temperature and density of the gas in the container are the same, that is, ρ and T are the same
And ∵ R is a constant
When the molecular weight m of the three gases is large, the pressure P is small
M oxygen > m neon > m hydrogen
P oxygen ＜ P neon ＜ P hydrogen

A chemical formula related to volume temperature density pressure

PV=nRT
v: Volume

The relationship between pressure, volume and temperature of gas
In an adiabatic cylinder, a sealed piston is used to seal a certain mass of gas. Now the piston is pressed down for a certain distance by an external force. After the external force is removed, the piston and the heavy object are gradually raised due to the expansion of the gas
A. Gas pressure unchanged B, gas pressure decreased C, gas temperature increased D, gas temperature decreased
There are different ideal gases in the two containers. Their mass, temperature and pressure are the same, but their volumes are different
A. The number of molecules per unit volume is equal. B. the mass of gas per unit volume is the same. C. the number of moles per unit volume is the same. D. the internal energy of gas per unit volume is the same
I hope to explain why
Who can give a positive answer

Question 1 BD question 2 AC