A 100 g piece of copper, initially at 95,0 C ,
is dropped into 200 g of water. If initial temperature of
water is 1 5 C, what is final temperature of the system, if the heat lost to surounding is ignored

please, step by step solution.

Physical Chemistry:

Calculate ΔG for the isothermal compression of 10.0 g of water from 1.0 atm to 100.0 atm at 25°C

What is the total enthalpy change when 100.0 g of solid NH3 at -150.0 degrees Celcius is changed to gas at 100 degrees Celcius?

I've done this problem several times and keep getting the answer of 223 kj, but in class we were told the correct answer is 237 kj. Please show all your steps/work so I can see what I'm doing wrong. Thank you!

Calculate the mass of methane that must be burned to provide enough heat to convert 266.0 g of water at 39.0°C into steam at 110.0°C. (Assume that the H₂O produced in the combustion reaction is steam rather than liquid water.)

The enthalpy of fusion of titanium is 20.9 kJ/mol. How many grams of titanium can be melted by adding 58.0 kJ of energy to the metal at its melting point?

Determine the oxidation states of carbon in the following substances.

CH₄                      _________

CH₂Cl₂        _________

SiC            _________   

CF₂Cl₂                 _________

C₂H₆                    _________                      

C(s)             _________

C₄H₁₀                 _________

C₆H₁₂O₆     _________

CH₃CHO    ________

CO              _________

C₂H₄                    _________

CO₂                      _________

C₂H₂                    _________

CO₃^{2 -}                _________

What is the pH at the equivalence point in the titration of a 21.2 mL sample of a 0.319 M aqueous nitrous acid solution with a 0.408 M aqueous potassium hydroxide solution?

What is the pH of a 0.055 M solution of sodium cyanide (NaCN)? The K_a value for hydrocyanic acid (HCN) is 6.2 x 10^-10.

Select one:

a. 10.97

b. 10.08

c. 8.77

d. 3.03

e. 5.23

For the diprotic weak acid H2A, Ka1 = 2.2 × 10-6 and Ka2 = 8.3 × 10-9. What is the pH of a 0.0700 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?

Choose the correct definition for an intrinsic semiconductor with an example.

1. a conductive material of an element with the addition of dopant (0.0001% Si in Al )
2. a conductive material of an element with the addition of dopant (0.0001% Al in Si )
3. a material that naturally can have electrons move across the band gap ( Al )
4. a material that naturally can have electrons move across the band gap (pure silicon)

Choose the correct definition for an extrinsic semiconductor with an example.

1.a conductive material of an element with the addition of dopant (0.0001% Si in Al )
2.a material that naturally can have electrons move across the band gap (pure silicon)
3.a conductive material of an element with the addition of dopant (0.0001% Al in Si )
4.a material that naturally can have electrons move across the band gap ( Al )

Match Column B Items with Column A Items ( match B is from A-i will be matched with column A)

Column A

______Reagents used to prepare the nonMarkovnikov product

______Reagent used to prepare an epoxide

_______Reagent used to carry out vigorous oxidation

______Reagent used to form dichlorocarbene

______Reagents used to convert alkynes to methyl ketones

____1,1-disubstituted substituents

______1,2- disubstituted substituents

Column B

a. KOH b. m-chloroperoxybenzoic acid c. hot alkaline Mn04- d.NaNH2 e. Vicinal

Methanol (CH₃OH) is made by reacting gaseous carbon monoxide (CO) and gaseous hydrogen (H₂).

A. What is the theoretical yield of methanol if you react 37.5 kg of CO(g) with 4.60 kg of H₂(g)?

B. You found that 1.83 x 10⁴ g of methanol is actually produced. What is the percent yield of methanol?

31. Which of the following describes the distribution of the polar and nonpolar portions of lipids in the lipid bilayer? A). Both polar heads are on the inside of the bilayer and both hydrophobic tails are on the outside of the bilayer. B). Both polar heads are on the outside of the bilayer and both hydrophobic tails are on the inside of the bilayer. C). Both the inside and outside of the bilayer consist of alternating polar heads and nonpolar tails. D). Some polar heads are on the inside of the bilayer and some are on the outside; the hydrophobic tails are similarly distributed.

33. Which describes the isoelectric point of an amino acid? A). The degree of ionization of the amino acid at pH 7. B). The pH at which there is no net charge for the amino acid. C). The pH at which the ionized form predominates. D). The pH at which the amino acid is present as the dipolar ion. CH2 – CONH2 

34. Asparagine (Asn) has an isoelectric point (pI) of 5.4, (H3N+ ¾CH¾COO- ). Select the correct Zwitterion structure of asparagine in a solution with a pH of 10. CH2 – CONH2 CH2– CONH2   A). H2N¾CH¾COO- B). H3N+ ¾CH¾COOH CH2– CONH2 CH2– CONH2   C). H2N¾CH¾COOH D). H3N+¾CH¾COO-

35. Which functional group is involved in linking together the amino acids of proteins? A). amine B). anhydride C). carbonyl D). carboxyl

36. Select the correct three-letter abbreviation for the order of amino acids in this tripeptide. O H O H O      H3N+  CH  C  N  CH  C  N  CHCO-    CH2OH CH3 H A). AlaGlySer B). GlySerAla C). SerAlaGly D). AlaSerGly

37. The secondary structure of proteins depends primarily on which property of amino acids? A). disulfide bonds B). hydrogen bonds C). amide bonds D). polar side chains

38. The beta-pleated sheet represents what level of protein structure? A). Primary B). Secondary C). Tertiary D). Quaternary

39. The following will denature proteins EXCEPT A). Agitation B). Acids and bases C). Heavy metal ions D). Freezing temperature

40. Which of the following is a structural protein? A). cellulose B). collagen C). hemoglobin D). insulin

41. In which of the following is the amino nitrogen also part of the side chain? A). cysteine B). glycine C). proline D). tryptophan

Part A. What mass of carbon dioxide is produced from the complete combustion of 5.70×10⁻³ g of methane?

Part B. What mass of water is produced from the complete combustion of 5.70×10⁻³ g of methane?

Part C. What mass of oxygen is needed for the complete combustion of 5.70×10⁻³g of methane?

Express your answer with the appropriate units.