why did some particles pass through the foil undeflected.

why did some particles pass through the foil and get partially deflected

why did some particles hit the foil and deflect backwards

Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Cl2(g) S2Cl2(g) + CCl4(g) When 2.94 mol of CS2 and 5.60 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.580 mol of CCl4. How many moles of Cl2 are present at equilibrium?

Solid HgO, liquid Hg, and gaseous O2 are placed in a glass bulb and the reaction below is allowed to reach equilibrium.
2HgO(s)
2Hg(l) + O2(g); ΔH = +181.6 kJ
With the system at equilibrium, the amount of Hg(l) in the bulb can be increased-
A) by removing some HgO(s). B) by adding an inert gas.
C) by adding some HgO(s). D) by increasing the pressure.
E) by increasing the temperature.

i have data, Acid is HCl and base is NaOH

△H=mC_h2o(T_i-T_f)

i am looking for the mass(m) please explain this..

1. Explain the issue on either increasing or decreasing the number of nuclear reactors used for generating energy in the US.

2.A number of European countries that lack access to oil and gas reserves are implementing smaller (and newer) nuclear reactors. How do these reactors diminish the risks of nuclear energy? If the US were to adopt these, what will happen?

11. Use equations (9.15), (9.22) and (9.23) to construct a concordia diagram for 3500 Ma of Earth history. Begin with 1000 atoms each of ²³⁵U and ²³⁸U at an initial time of 0 years, and increment time in 200 Ma increments, calculating N (the number of atoms remaining) and D* (the number of daughter isotopes = N_o-N) for both decay schemes at each increment. Then plot ²⁰⁷Pb/²³⁵U vs. ²⁰⁶Pb/²³⁸U to construct a concordia diagram.

Once you have a diagram, add the following points as a discordia:You can add the points in Excel by copying them, selecting the chart, and using Paste-Special as a new series. Draw a best-fit line through the discordia points and estimate the initial crystallization age and the metamorphic age.

A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and 100 mL of .001 M NaF. Will PbF2(s) precipitate in this reaction? Calculate the concentration of F- ions present at equilibrium.

PbF2(s) <--> Pb2+(aq) + 2F-(aq) Kc= 3.7E-8

Please show all work! Thank you!

1.How many mL of 0.500 M HCl should be added to 155 mL of 0.0500 M benzylamine to form a buffer with pH = 8.52? C7H7NH2 pKb = 4.35 C7H7NH2 (aq) + H+ (aq)  C7H7NH3 + (aq) This structure of benzylamine has a carbon at the junction of each line with 1 hydrogen on each 3-bonded ring C and 2 hydrogens on the C in the side chain attached to the ring carbon. Note that the N atom has 3 bonds and a lone pair.

2.Write the formula for the conjugate acid of benzylamine.

A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of .5 M NaF. Calculate the concentration of F- ions present at equilibrium. (Hint: First, write and balance the double displacement reaction taking place between Pb(NO3)2 and NaF to form PbF2(s). Perform the necessary stoichiometry (including finding which reactant is limiting) to calculate how much of each reactant remains after the reaction goes to completion. Remember that stoichiometry has to be done in moles. Once you have calculated how much of each reactant remains, then calculate the concentration of Pb2+ and F- remaining in solution, and use those as your initial concentrations for the equilibrium calculation using the reaction below.) (In essence, we are assuming that the reaction goes to completion first, and then we are letting it come back to equilibrium.) PbF2(s) <--> Pb2+ (aq) + 2F- (aq) Kc=3.7E-8

hypophosphate ion(H2PO2-) decomposes in alkaline solution as a result of the folowing reaction.

H2PO2-+OH-----HP032-+H2

the kinetic of this reaction were bstudied at 100 deg c.the following table lists the initial concentations of the reactants(from three seperate experiment)and the concentrationof one of the product(HPO32- after the reaction has run for 30 seconds

a)complete the chart by calculating the initial rate for each expriment (don not forget to include units).hints what is initial concentration of the product? what is the delta t?how is the rate related to product change in concentration?

b) determine the rate law for this reaction.

c)determine the value and units of the rate constant.

d)calculate the rate of reaction if [H2PO2-]I=0.20M and[OH-]I=0.30M

1.A mixture of argon and xenon gases contains argon at a partial pressure of 450 mm Hg and xenonat a partial pressure of 523 mm Hg. What is the mole fraction of each gas in the mixture?

X_Ar =
X_Xe =

2.
A mixture of nitrogen and oxygen gases at a total pressure of 912 mm Hg contains nitrogen at a partial pressure of 340 mm Hg. If the gas mixture contains 3.95 grams of nitrogen, how many grams of oxygen are present?

_____g O₂

_3.

The stopcock connecting a 3.99 L bulb containing nitrogen gas at a pressure of 8.46 atm, and a 7.52L bulb containing oxygen gas at a pressure of 2.15 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is_____ atm.

Tell how UV-vis spectrometry can be used to differentiate the following compounds. Calculate approximate ymax values for each compound when you can.

a) 1,4 hexadiene, 2,4-hexadiene, and 1,3 hexadiene

b) cyclohexanone, 2-cyclohexenone, and 2,4-cyclohexadienone

What is the pH at the quivalence point when 50.0 mL of 0.10 M ethylamine (C₂H₅NH₂) is titrated with 0.20 M HCLO₄? (K_b of C₂H₅NH₂ = 5.6 x 10^-4) (Hint: You will need to determine the volume of HCLO₄ solution used) Be sure to show ICE table.

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide in the following fashion:
CH3COOH(aq)+NaOH(aq)→H2O(l)+NaC2H3O2(aq)

1.) If 3.55 mL of vinegar needs 43.0 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.10 qt sample of this vinegar?

The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous solution. The Henry’s Law constant in this case is 3.0 x 10-2 mol/L.atm.

A) Please find the partial pressure of CO2 (g) (PCO2, in atm) in the air above the lake.

B) Please use your answer to determine the percentage of CO2 in the atmosphere.

C) Given the percentage of CO2 in the atmosphere is constant at sea level and below, please calculate the solubility (moles/liter of aqueous solution) of CO2 in the Dead Sea at 298 K and a pressure of 800 torr.

Thank you!