In this question, you are given the NaOH volume but asked for concentration.
Don't forget that for every 1 mol of NaOH there will be 1 mol OH- ion, but for every 1 mol of H2SO4 there will be 2 mol of H- ion.
To neutralize you need the same amount of OH- and H+, so the equation should be:
OH-= H+
<span>35.50cm3 * x*1= 25cm3* 0.2mol/dm3 *2
</span>x= 10/35.5 mol/dm3= 0.2816/dm3
Answer:
110.8 ºC
Explanation:
To solve this problem we will make use of the Clausius-Clayperon equation:
lnP = - ΔHºvap/RT + C
where P is the pressure, ΔHºvap is the enthalpy of vaporization, R is the gas constant, T is the temperature, and C is a constant of integration.
Now this equation has a form y = mx + b where
y = lnP
x = 1/T
m = -ΔHºvap/R
Now we have to assume that ΔHºvap remains constant which is a good asumption given the narrow range of temperatures in the data ( 104-125) ºC
Thus what we have to do is find the equation of the best fit for this data using a software as excel or your calculator.
T ( K) 1/T ln P
377 0.002653 5.9915
384 0.002604 6.2115
390 0.002564 6.3969
395 0.002532 6.5511
398 0.002513 6.6333
The best line has a fit:
y = -4609.5 x + 18.218
with R² = 0.9998
Now that we have the equation of the line, we simply will substitute for a pressure of 496 mm in Leadville.
ln(496) = -4609.5(1/Tb) + 18.218
6.2066 = -4609.5(1/Tb) +18.218
⇒ 1/Tb = (18.218 - 6.2066)/4609.5 = 0.00261
Tb = 383.76 K = (383.76 -273)K = 110.8 ºC
Notice we have touse up to 4 decimal places since rounding could lead to an erroneous answer ( i.e boiling temperature greater than 111, an impossibility given the data in the question). This is as a result of the value 496 mmHg so close to 500 mm Hg.
Perhaps that is the reason the question was flagged.
Answer:If a bouncing ball has a total energy of 20 J and a kinetic energy of 5 J, the ball’s potential energy is 15J.
If the kinetic energy of the ball decreases, then the potential energy will Increase.
Explanation:
Answer:
A polar molecule is a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative. A diatomic molecule that consists of a polar covalent bond, such as HF, is a polar molecule. The two electrically charged regions on either end of the molecule are called poles, similar to a magnet having a north and a south pole. A molecule with two poles is called a dipole. Hydrogen fluoride is a dipole. A simplified way to depict polar molecules is pictured below When placed between oppositely charged plates, polar molecules orient themselves so that their positive ends are closer to the negative plate and their negative ends are closer to the positive plate
Experimental techniques involving electric fields can be used to determine if a certain substance is composed of polar molecules and to measure the degree of polarity.
For molecules with more than two atoms, the molecular geometry must also be taken into account when determining if the molecule is polar or nonpolar. is a comparison between carbon dioxide and water. Carbon dioxide (CO2) is a linear molecule. The oxygen atoms are more electronegative than the carbon atom, so there are two individual dipoles pointing outward from the C atom to each O atom. However, since the dipoles are of equal strength and are oriented in this way, they cancel each other out, and the overall molecular polarity of CO2 is zero.
Water is a bent molecule because of the two lone pairs on the central oxygen atom. The individual dipoles point from the H atoms toward the O atom. Because of the shape, the dipoles do not cancel each other out, and the water molecule is polar. In the figure, the net dipole is shown in blue and points upward.
Some other molecules are shown below (Figure below). Notice that a tetrahedral molecule such as CH4 is nonpolar. However, if one of the peripheral H atoms is replaced by another atom that has a different electronegativity, the molecule becomes polar. A trigonal planar molecule (BF3) may be nonpolar if all three peripheral atoms are the same, but a trigonal pyramidal molecule (NH3) is polar.
Let's assume that the gas has ideal gas behavior.
Then we can use ideal gas equation,
PV = nRT
Where, <span>
P = Pressure of the gas (Pa)
V = volume of the gas (m³)
n = number of moles (mol)
R = Universal gas constant (8.314 J mol</span>⁻¹ K⁻¹)<span>
T = temperature in Kelvin (K)
<span>
The given data for the </span></span>gas is,<span>
P = 2.8 atm = 283710 Pa
V = 98 L = 98 x 10</span>⁻³ m³<span>
T = 292 K
R = 8.314 J mol</span>⁻¹ K⁻¹<span>
n = ?
By applying the formula,
283710 Pa x </span>98 x 10⁻³ m³ = n x 8.314 J mol⁻¹ K⁻¹ x 292 K
<span> n = 11.45 mol
Hence, moles of gas is </span>11.45 mol.
