C6H12O6(s) + 9 O2(g)
-> 6 CO2(g) + 6 H2O(g)
There are 9 moles of O2 needed for the complete combustion of glucose.
Answer : Option A) Molecules are speeding up during boiling.
Explanation : As shown in the above image it is clearly observed that the molecules are been transformed from liquid to gaseous state. Which means that the intermolecular distance between the molecules is increasing as they are boiling and getting transformed into gaseous form. They are speeding up to form gas from liquid state and achieve stability as the heat is supplied in greater amount. Boiling of liquid is causing the liquid molecules to speed up and get transformed into gaseous molecules.
Respuesta:
2 m
Explicación:
Paso 1: Información provista
- Volumen inicial (V₁): 100 mL
- Concentración inicial (C₁): 4 m
- Volumen final (V₂): 200 mL
- Concentración final (C₂): ?
Paso 2: Calcular la concentración de la solución final
Queremos perparar una concentración diluida a partir de una concentrada. Podemos calcular la concentración de la solución diluida usando la regla de dilución.
C₁ × V₁ = C₂ × V₂
C₂ = C₁ × V₁ / V₂
C₂ = 4 m × 100 mL / 200 mL = 2 m
Answer:
0.047
Explanation:
Data : 5g , Na2CO3
Formula:
Molecular mass of Na2Co3 = no.of atomic mass x no. of atom
moles = mass÷ molecular mass
molecular mass = 2(23)+1(12)+3(16)
=106amu
moles = 5÷106
= 0.047 Ans:
Answer:
1. A. True
2. A. True
3. B. False
4. A. True
5. B. False
Explanation:
1. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas. A. True. The pressure of an ideal gas is higher than the one that would exert a real gas.
2. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other. A. True. The intermolecular forces are negligible.
3. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be about 1 mL. B. False. The volume of the gas particles is negligible.
4. The molecules in a real gas have finite volumes and do exert forces on each other, thus real gases do not conform to some of the assumptions of an ideal gas as stated by the kinetic molecular theory. A. True. We cannot apply ideal gas laws to real gases.
5. The average kinetic energy of a collection of gas particles is assumed to be inversely proportional to the Kelvin temperature of the gas. B. False. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.
