in a certain operation 3.54*10⁴ kg of Ticl4 is reacted with 1.13*10⁴ kg of Mg

A) Calculate the theoretial yield of titanium , Ti in kilograms.

B ) Calculate the percent yield if 7.91*10³ kg of Ti is actually obtained

(Ti : 47.88 , Mg: 24,3, Cl; 35.5)

Help please with explain every thing :)

Write the equations for the reaction of the following Bronsted acids with water:

(a) HCO2H (b) NH3OH+ (c) HClO4

Write equations for the reactions of the following Bronsted bases with water:

(a) C H NH (b) HPO 2- (c) HCO -

Calculate ?G

Should Toluene have reacted with Sulfuric Acid, KMnO4, and 2% Bromine? Reaction?

I performed these tests in the lab but got negative results for all three. I think I didn't shake them enough because the double bonds should've gone some addition reaction, right?

Complete combustion of methane

When methane (CH4CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is

CH4(g)+O2(g)→CO2(g)+H2O(g)CH4(g)+O2(g)→CO2(g)+H2O(g)

This type of reaction is referred to as a complete combustion reaction.

Part A

Part complete

What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4CH4, O2O2, CO2CO2, and H2OH2O, respectively.

Express your answer as four integers, separated by commas (e.g., 1,2,3,4).

View Available Hint(s)

1,2,1,2

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Correct

Part B

What mass of carbon dioxide is produced from the complete combustion of 1.80×10⁻³ gg of methane?

Express your answer with the appropriate units.

Part C

What mass of water is produced from the complete combustion of 1.80×10⁻³ gg of methane?

Express your answer with the appropriate units.

Part D

What mass of oxygen is needed for the complete combustion of 1.80×10⁻³ gg of methane?

Express your answer with the appropriate units.

In 0.100 M CH3NH2, only 6.4% of the base has undergone ionization. Calculate the pKb of methylamine.

The answer is 3.36 but I have no idea how to get it. Please show steps. Thanks!

i. NIST-traceable standard metal ion solutions are provided. The standard metal ion solutions are each 1000 ppm. Compute how much of the NIST-traceable solution you will use to prepare 100 mL of a

A 1.000 gram organic sample containing nitrogen is subjected to Kjeldahl analysis. The ammonia gas generated when ammonium is neutralized is distilled into 50.00 mL of 0.1000 M HCl to reform ammonium. If 17.29 mL of 0.1000 NaOH is required to titrate the unreacted HCl, calculate the percent by mass nitrogen in the original sample.

Solvent vessels must be purged before maintenance personnel enter in order to ensure that: (1) sufficient oxygen is available for breathing; (2) vapor concentrations are below the flash point; (3) vapor concentrations are below the Occupational Safetey and Health Administration (OSHA) limits if breathing apparatus is not to be used. Assuming that a 8 m^3 fixed-roof solvent tank has just been drained of all liquid and that the vapor phase is initially saturated at 22 degrees celsius, estimate the length of purge necessary with 2 m^3/min of gas at 0.1 MPa and 22 degrees celsius to reach the OSHA 8-hr exposure limit.

(a) Choloroform 50 ppm

Aqueous hydrochloric acid

HCl

reacts with solid sodium hydroxide

NaOH

to produce aqueous sodium chloride

NaCl

and liquid water

H2O

. If

0.314g

of water is produced from the reaction of

0.73g

of hydrochloric acid and

1.3g

of sodium hydroxide, calculate the percent yield of water.

Be sure your answer has the correct number of significant digits in it.

A.) Calculate the pH of 1.0 L of the solution, upon addition of 49.00 mL of 1.0 MHCl.

Calculate the pH of the solution upon addition of 19.1 mL of 1.00 MHCl to the original buffer

B.)For each of the following solutions, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.

1.) 300.0 mL of pure water

2.)300.0 mL of a buffer solution that is 0.210 M in HCHO2 and 0.290 M in KCHO2

3.)300.0 mL of a buffer solution that is 0.295 M in CH3CH2NH2 and 0.270 M in CH3CH2NH3Cl

1. The equilibrium constant, K_p, for the following reaction is 10.5 at 350 K:

2CH₂Cl₂(g) <--->CH₄(g) + CCl₄(g)

Calculate the equilibrium partial pressures of all species when CH₂Cl₂(g) is introduced into an evacuated flask at a pressure of 0.865 atm at 350 K.

2. The equilibrium constant, K_p, for the following reaction is 0.215 at 673 K:

NH₄I(s) <----> NH₃(g) + HI(g)

Calculate the equilibrium partial pressure of HI when 0.413 moles of NH₄I(s) is introduced into a 1.00 L vessel at 673 K.

P_HI = ____atm

1. VOLUME TECHNIQUE: This method is based on the volume of carbon dioxide produced and collected.
2. MASS TECHNIQUE: This method is based on the difference in mass before and after the reaction.

The mass of carbon dioxide calculated using the volume technique will not be identical to the mass of the carbon dioxide calculated using the mass technique. In this discussion, compare and contrast the two techniques and the mass of carbon dioxide obtained by each technique. Also discuss reasons for the difference in masses.

Briefly explain what you would observe if you used the test described in (a) on a solution that needed more NaOH solution

A 39.0%/61.0% by volume propane/n-butane mixture is cooled from 291°C to 115°C. Assume ideal behavior.

a) What is the average molar mass of the mixture?

b) What is the change in specific enthalpy of pure propane from 291°C to 115°C?

c) What is the change in specific enthalpy of pure n-butane from 291°C to 115°C?

d) What is the change in specific enthalpy of the mixture from 291°C to 115°C?

e) What is the change in enthalpy of the mixture from 291°C to 115°C in kJ/kg?