A tank of acetylene gas (C2H2) contains 52.0lb of the gas and is at a pressure of 511.2lb/in.2 .
Express the pressure of the gas in atmospheres. 760 mmHg= 14.696 lb/in.2.

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.
2Al(s)+3Cl2(g)→2AlCl3(s)

1) 7.7 g Al, 24.4 g Cl2

Express your answer using three significant figures.

2)0.230 g Al, 1.15 g Cl2

Express your answer using three significant figures.

How are Cu2+ and Bi3+ separated from Pb2+ and How can Bi3+ be separated from Cu2+?

Consider a titration involving 40.0 mL of 0.100 M ammonia , NH₃ (in an Erlenmeyer flask)with 0.100 M HCl (in a burette) to answer the next two questions.

NH₃ + HCl

A buffer solution is prepared by mixing 20.0 mL 0.45M HAc (acetic acid) with 35.0 mL 0.45M NaAc (sodium acetate)

(a) What is the amount of 4.0M HAc which must be added to this buffer solution to double [H3O+]?

(b) What is the amount of 2.0M HCl that must be added to decrease the pH by 0.50?

(c) How much NaOH(s) in g has to be added to the solution to raise the pH by 2.00?

The decomposition of Ethylene oxide, (CH2)2 O(g), at 652k is a 1st- order reaction with R=0.012 min^-1 and an activation energy of 218k J/mol (CH2)2 O(g) -----> CH4(g)+ CO (g)

Calculate a) the rate constant of reactin at 525k and b) the temperature at which the rate constant R=0.01min^-1 (universal gas constant R=8.314 J/mol^-1 k^-1)

Phosphine decomposes by the following reaction:

COCl_2(g) <---> CO_(g) + Cl_2(g) K_c = 8.3 x 10^-4

Calculate the concentration of each component when 2.55 g of phosphine decomposes in a 25.0mL flask.

An aqueous solution containing 5.99 g of lead(II) nitrate is added to an aqueous solution containing 5.04 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states.

balanced chemical equation:

Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq)Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq)

What is the limiting reactant?

The percent yield for the reaction is 83.2%. How many grams of the precipitate are formed?

How many grams of the excess reactant remain?

If the Ka of a monoprotic weak acid is 6.6×10−6, what is the pH of a 0.29 M solution of this acid?

The Ka of a monoprotic weak acid is 0.00604. What is the percent ionization of a 0.114 M solution of this acid?

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0154 M solution. The pH of the resulting solution is 2.38. Calculate the K_a for the acid.

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0186 M solution. The pH of the resulting solution is 2.60. Calculate the pKa for the acid.

If 4.90 g of Na₂CO₃ is dissolved in enough water to make 250. mL of solution, what is the molar concentration of the sodium carbonate?

Molar concentration of Na₂CO₃ = ______M

What are the molar concentrations of the Na⁺ and CO₃^2- ions?

Molar concentration of Na⁺ = ______M

Molar concentration of CO₃^2- = _______M

Balance each redox reaction occurring in acidic aqueous solution. Use the half-reaction method. Identify all phases in answer

A) IO3-(aq)+SO2(g)-------> I2(s)+SO4^2-aq)     B) Cr2O7^2- (aq) + Br- (aq)-----------> Cr^3+(aq) + Br(aq)

How many milliliters of 0.640 M HCl are needed to titrate each of the following solutions to the equivalence point?

(a) 30.2 mL of 0.640 M LiOH

_________ mL

(b) 60.8 mL of 0.768 M NaOH

________ mL

(c) 464.0 mL of a solution that contains 6.56 g of RbOH per liter

________ mL

Problem 4.26a Draw all possible structure(s) and give the IUPAC systematic name(s) of an alkane or cycloalkane with the formula C8H18 that has only primary hydrogen atoms. Select the IUPAC systematic name(s) (all drawn in previous step): 2,2,3-trimethylpentane octane 2,3-dimethylhexane 2-methylheptane methylcycloheptane 2,2,3,3-tetramethylbutane 1-methyl-2-ethyl-pentane 2,2-dimethylhexane

how can i Calculate those ??

1)Mass of Cu wire reacted

2)Mass of Ag produced

3)Mass of AgNO3 reacted

4)Moles of Cu reacted

5)Moles of AgNO3 reacted

6)Moles of Ag produced

7)Ratio of moles Ag to moles AgNO3

8)Ratio of moles Ag to moles Cu

9)Number of Cu atoms removed from wire

10)Number of Ag atoms produced

11)Theoretical yield of Ag

12)% Yield of Ag

A reaction is carried out by combining 65.00 mL of a 0.108 M sample of (NH4)3PO4 and 48.00 mL of a 0.230 M Fe9NO3)2 solution. The net ionic equation is :

3Fe^2+(aq) + 2PO4^3-(aq) ---> Fe3(PO4)2(s) balanced

1a) What is the mass of iron(II) phosphate (MM= 357.49 g/mol) produced in the reaction?

1b) What are the concentrations of the reacting ions (Fe^2+(aq) and PO4^3+(aq)) at the end of the reaction (assuming no change in volume)?