1.question, 2.observe, 3.hypothesize, 4.experiment 5.conclusion, 6. record.
It stays roughly the same size. Electrons have a barely imperceptible mass so the overall mass of the atom is changed very little.
Answer:
A liquid, at any temperature, is in equilibrium with its own steam. This means that on the surface of the liquid or solid substance, there are gaseous molecules of this substance. These molecules exert a pressure on the liquid phase, a pressure known as vapor pressure.
In chemistry, when we talk about dry basis, we talk about a state in which the presence of water in a gaseous state is denied for the calculation. So vapor pressure equals zero.
When we talk about the wet basis, the presence of water in the steam is considered for the calculation, which normally is expressed as a percentage or moisture.
In summary, for a gas mixture steam:
- For dry basis, we just have <em>component A, component B....</em>
- For wet basis, we have <em>water vapor, component A, component B...</em>
So, in wet basis we have an extra component (water).
Assuming we only have 2 components in our steam, and being X the molar fraction of eact component:
- For dry basis: Xa + Xb = 1................................. Xa = 1 - Xb
- For wet basis: Xa + Xb + Xwater = 1 .............Xa = 1 - Xwater - Xb
For dry basis the mole fraction of A it is obtained by subtracting the molar fraction of B from one. And for wet basis, we have to substract the molar fraction of B <u>AND </u>the molar fraction of water vapor. So, logically, the mole fraction Xa will be less for wet basis.
Answer:
We need 42.4 mL of benzene to produce 1.5 *10³ kJ of heat
Explanation:
<u>Step 1:</u> Data given
Density of benzene = 0.88 g/mL
Molar mass of benzene = 78.11 g/mol
Heat produced = 1.5 * 10³ kJ
<u>Step 2:</u> The balanced equation
2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ
<u>Step 3:</u> Calculate moles of benzen
1.5 * 10³ kJ * (2 mol C6H6 / 6278 kJ) = 0.478 mol C6H6
<u>Step 4:</u> Calculate mass of benzene
Mass benzene : moles benzene * molar mass benzene
Mass benzene= 0.478 * 78.11 g
Mass of benzene = 37.34 grams
<u>Step 5:</u> Calculate volume of benzene
Volume benzene = mass / density
Volume benzene = 37.34 grams / 0.88g/mL
Volume benzene = 42.4 mL
We need 42.4 mL of benzene to produce 1.5 *10³ kJ of heat
The first solution or a I think is the correct answer