I need help with all of these to see if I got them right on the test. So if some

Question

I need help with all of these to see if I got them right on the test. So if someone could help me solve these and show me how I would really appreciate it. I'm struggling this is for a review.



1.50 g piece of copper metal is placed in 185 mL of a 0.236 M AgNO3 solution. 2Ag(s) + The net ionic equation is: Cu(s)+ 2Ag'(aq) is the mass of silver metal produced in the reaction? balanced. A What B. What is the concentration of the copper(il) ion produced (assuming no change in volume)? using the Kinetic Molecular Theory, explain why the relationship is such. pressure was changed from 4.26 to 3.74 atm, while () the temperature was changed Identify how the pressure and temperature of a gas sample is related and then, A 4.0 L sample of an ideal gas was subjected to the following changes () the from 66.4°C to 25.0°C. Determine the final volume Silane (SiH4), phosphine (PHs), and hydrogen sulfide (H2S) melt at -185°C, -133°C, and -85°C, respectively. What does this suggest about the types of intermolecular forces present in each of the three compounds? What is the rate of effusion for the lightest gas (H2) to the heaviest (UFs)? Provide a brief explanation for the following using complete sentences though not at the expense of clarity or completeness. A. Explain why the vapor pressure of liquids change as temperature increases. B. A glass of cold milk sometimes forms a coat of water on the outside of the glass (often referred to as 'sweat). How does most of the water get there? C. Use sketches to illustrate how London dispersion forces arise in a molecule or atom. What is the boiling point of water if the atmospheric pressure is 3.0 atm? For water, the enthalpy of vaporization is 40.7 kJ/mol. An element crystallizes in a face-centered cubic unit cell that has an edge length of 3.615 A and a density of 8.935 g/cm3 Identify the element and determine the atomic radius What mass of water is needed to dissolve 34.8 g of copper(ll) sulfate in order to dso prepare a 0.521 m solution? A solution contains 21.6 g of a nonelectrolyte and 175 g of water. The water 1.86°C/m. Is the nonelectrolyte CH3OH or C2H5OH? freezes at-718°C and Kr

Explanation / Answer

Q1 Solution :-

1.5 g Cu

185 ml of 0.236 M AgNO3

Mass of Ag metal = ?

Concentration of the Cu^2+ = ?

Reaction equation

Cu(s) + 2Ag^+(aq) ----- >2Ag(s) + Cu^2+

Now lets calculate moles of Cu

Moles = mass/ molar mass

Moles of Cu = 1.5 g / 63.546 g per mol = 0.0236 mol Cu

Moles of Ag^+ = molarity * volume

                          = 0.236 mol per L * 0.185 L

                          = 0.04366 mol Ag^+

Now lets calculate the moles of the Ag metal produced

0.0236 mol Cu * 2 mol Ag / 1 mol Cu = 0.0472 mol Ag

0.04366 mol Ag^+ * 2 mol Ag / 2 mol Ag^+ = 0.04366 mol Ag

Since moles of Ag metal produced from the Ag^+ is less than Ag produced from the Cu therefore the silver nitrate is the limiting reagent

So the maximum moles of Ag that can be produced = 0.04366 mol

Now lets convert moles of Ag to its mass

Mass = moles * molar mass

Mass of Ag = 0.04366 mol * 107.87 g per mol

                     = 4.71 g Ag

Now lets calculate the concentration of the Cu^2+ ions

0.04366 mol Ag^+ * 1 mol Cu / 2 mol Ag^+ = 0.02183 mol Cu^2+

Now lets calculate its concentration

Molarity = moles / volume in liter

Concentration of Cu^2+ = 0.02183 mol / 0.185 L

                                             = 0.118 M

Q2 Solution

When the amount of the gas and the volume is constant then the pressure and temperature are directly proportional to each other.

As the Temperature of the gas increases then pressure also increases an d vice versa

As per the kinetic molecular theory of the gases

As the temperature of the gas increases then the collisions between the gas molecules and the wall of the container increases which creates more pressure on the wall of the container.

Q3 solution:-

Given data

V1 = 4.0 L

Pressure P1 =4.26 atm

Pressure P2 =3.74 atm

Temperature T1 =66.4 C +273 = 339.4 K

Temperature T2 = 25.0 C +273 = 298 K

V2 = ?

Using the combined gas law equation we can calculate the final volume of the gas

Formula

P1V1/T1 = P2V2/T2

Rearranging this formula we get

V2 = P1*V1*T2 / T1*P2

Lets put the values in the formula

V2 = 4.26 atm *4.0 L*298 K/ 339.4 K * 3.74 atm

V2 = 4.0 L

So the final volume of the gas is remain as 4.0 L

Q4 Solution :-

SiH4 , PH3 and H2S

melting points are -185 C , -133 C and -85 C

From the melting points of the compounds listed above we can conclude that the intermolecular forces are stronger in the H2S and weakest in the SiH4.

Because the melting points of the compounds are dependent on the intermolecular forces. As the intermolecular strength increases then it will increase the melting point of the compound.

SiH4 have dispersion forces

PH3 have dipole dipole interactions

H2S have the dipole dipole interactions.

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