In a constant-pressure calorimeter, 75.0 mL of 0.830 M H2SO4 was added to 75.0 mL of 0.400 M NaOH. The reaction caused the temperature of the solution to rise from 21.85 °C to 24.57 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

Acid base titration determination of Na2CO3 in Soda Ash

CO3^2- +H⁺ = HCO3^-

HCO3^- + H⁺ = H2CO3

Buffer by mixing acetic acid and sodium acetate.

The comparison indicator solution should match the analytical solution at the second equivalence point in three respects: pH, Ionic strength, color and intensity

A) Calculate the concentration of sodium acetate necessary to achieve the ionic strength in pre lab 4. ( Pre lab 4 calulation, the ionic strength that I have calculated is to be 0.1)

B) Calculate the concentration of acetic acid given the values calculated for A.

C) Calculate the mass of unknown to weight out in order to consume 40 ml of 0.1 M HCL assuming the unknow is 35% by mass Na2CO3.

For preview calculation where you calculate the mass of Na2CO3 needed to consume 40 mL of 0.10 M HCL in a titration of Na2CO3 with HCL come out to be 0.212 gram needed to consume 40 mL of 0.10 M of HCL.

"monoclonal antibody can be used as a therapeutic agent for the treatment of cancer"- justify the statement with an appropriate example

If the weight of an unknwon sample is greater than 1g, as it may be with pottassium phthalate samples of low percentage purity, why does this sample need only to be weighed to the nearest milligram?

Evaluate the physical and chemical methods of waste treatment? How efficient are they in and what is their effect on the environment (positive and/or negative)?

B.) Enter the net ionic equation representing aqueous acetic acid neutralized by aqueous barium hydroxide.   

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.\

C.) Enter the molecular equation representing solid chromium (III) hydroxide reacting with nitrous acid.   

Express your answer as a balanced molecular equation. Identify all of the phases in your answer.

D.) Enter the net ionic equation representing solid chromium (III) hydroxide reacting with nitrous acid.   

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.

E.) Enter the molecular equation representing aqueous nitric acid and aqueous ammonia reacting.

Express your answer as a balanced molecular equation. Identify all of the phases in your answer.

F.) Enter the net ionic equation representing aqueous nitric acid and aqueous ammonia reacting.  

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reactions of a number of such steps for methane gas is as follows:
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 165 mL of methane at STP, 865 mL of oxygen at STP, and 57.5 mL of NO at STP in a 2.2 −L flask. The reaction is allowed to stand for several weeks at 275 K.

A) If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K? (answer as follows: PCH4,PO2,PNO)

B) If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K? (answer as follows PCO2,PH2O,PNO2,POH)

C) What is the total pressure in the flask?

Sodium nitroprusside is ordered at 0.3 mcg/kg/min for a 220-lb patient. A vial containing 50 mg of sodium nitroprusside in 2 mL is diluted to 250 mL with NSI and ordered to run at 14 mL/h. Is this run rate correct? If not, what should be the correct infusion rate? The correct answer is no, and 9 mL/h. Please show how this problem is solved.

Though they are not necessary in every situation, solvents are used when performing reactions for many reasons. What function does a solvent serve in a reaction (list two)? What characteristics are important to consider when selecting a solvent (list two)? This is regards to organic chemistry, please explain your answers, please!

What are the factors influencing the transport and behaviour of wastes in the environment?

Enthalpy H is a measure of the energy content of a system at constant pressure. Chemical reactions involve changes in enthalpy, ΔH, which can be measured and calculated: ΔHrxn∘=∑productsmΔHf∘−∑reactantsnΔHf∘ where the subscript "rxn" is for "enthalpy of reaction" and "f" is for "enthalpy of formation" and m and n represent the appropriate stoichiometric coefficients for each substance. The following table lists some enthalpy of formation values for selected substances. Substance ΔHf∘ (kJ/mol) NaOH(aq) −469.1 MgCl2(s) −641.8 NaCl(aq) −407.3 Mg(OH)2(s) −924.5 H2O(l) −285.8 Part A Determine the enthalpy for this reaction: MgCl2(s)+2NaOH(aq)→Mg(OH)2(s)+2NaCl(aq) Express your answer in kilojoules per mole to one decimal place. ΔHrxn∘ = kJ/mol SubmitMy AnswersGive Up Part B Consider the reaction Mg(OH)2(s)→MgO(s)+H2O(l) with enthalpy of reaction ΔHrxn∘=37.5kJ/mol What is the enthalpy of formation of MgO(s)? Express your answer in kilojoules per mole to one decimal place. ΔHf∘ = kJ/mol Submit

Use the following information to answer questions 5-10. A student determined the heat of neutralization of copper (II) sulfate (CuSO4) mixed with potassium hydroxide (KOH) using the procedure described part 2 of this experiment. A 150.0 mL sample of a 1.50 M solution of CuSO4 was mixed with a 150.0 mL sample of 3.00 M KOH in a coffee cup calorimeter. The temperature of both solutions and the calorimeter was 25.2 °C before mixing and 31.3 °C after mixing. The heat capacity of the calorimeter is 24.2 J/K. Calculate the heat of reaction (ΔHrxn) for this reaction in units of J/mole of copper (II) hydroxide (Cu(OH)2). Assume the solution is dilute enough that the specific heat capacity and density of the solution is the same as that of water, 4.18 J/g∙K and 1.00 g/mL respectively. Calculate the number of moles of copper (II) hydroxide (Cu(OH)2) formed during this reaction. Assume the reaction goes to 100% completion.

Use data in Appendix C in the textbook to calculate ΔH∘ in (kJ/mol) , ΔS∘ in (j/mol-K) , and ΔG∘ in (kJ/mol) at 25 ∘C for each of the following reactions: 2P(g)+10HF(g)→2PF5(g)+5H2(g)

Appendix C:

P(g): dH:316.4; dG: 280.0; S:163.2

HF(g): dH: -268.61; dG: -270.70; S:173.51

PF5(g): dH:-1594.4; dG: -1520.7; S: 300.8

H2(g): dH:217.94; dG: 203.26; S: 114.60