Answer:
the mass of each gas
Explanation:
Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can differ between
the two gases?(1 point)
the gas constant of each gas
the molar volume of each gas
the mass of each gas
Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can differ between the two gases?(1 point) the gas constant of each gas the gas constant of each gas the molar volume of each gas the molar volume of each gas the mass of each gas the mass of each gas the number of moles of each gas
the number of moles of each gas
PV = nRT
The gases have the same P.V, T and n
R is constant AND SO constant for both
the only difference is the molar mass of the gas
for the same number of moles, the balloons will have different weights depending on the gas
so the answer is
the mass of each gas
Answer is: enthalpy is -1276,8 kJ.
Chemical reaction: 2CH₃OH(l) + 3O₂(g) → 2CO₂(g) + 4H₂<span>O(g).
</span>ΔH(CH₃OH) = -238,7 kJ/mol.
ΔH(H₂O) = -241,8 kJ/mol.
ΔH(CO₂) = -<span>393,5 kJ/mol.
</span>ΔH(O₂) = 0 kJ/mol.
ΔHreaction = ∑ΔHproducts - ∑ΔHreactants
ΔHreaction = (2·(-393,5) + 4·(-241,8) - (2·(-238,7))
ΔH = (-787 - 967,2) + 477,4
ΔH = -1276,8 kJ.
Answer:
1. 1g/ml
Explanation:
1. Density is mass divided by volume (g/mL).
10g/10mL = 1 g/mL
2. When you already know the density and the volume, you can use the density as a unit converter.
![5mL*\frac{20g}{mL} = 100g](https://tex.z-dn.net/?f=5mL%2A%5Cfrac%7B20g%7D%7BmL%7D%20%3D%20100g)
3. It's the same with density and mass.
![20g*\frac{1mL}{5g} = 4mL](https://tex.z-dn.net/?f=20g%2A%5Cfrac%7B1mL%7D%7B5g%7D%20%3D%204mL)
CO will diffuse faster than CO2 because its molar mass is smaller.
The rate of diffusion depends on molecular weight and the least mass will diffuse faster.