1. When chromium metal is added to nitric acid, the following reaction takes place Cr (s) + 6 HNO₃ (aq) → Cr(NO₃)₃ (aq) + 3 H₂O (l) + 3 NO₂ (g) Calculate the volume of NO₂ gas collected over water at 40.0 °C when 35.1 g of chromium is added to excess nitric acid if the total pressure is 675 torr. The vapor pressure of water at 40.0 °C is 55.3 torr.

and

2. How many grams of Al were reacted with excess HCl if 6.28 L of hydrogen gas were collected at STP in the following reaction? 2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)

1.

An aqueous solution of calcium hydroxide is standardized by titration with a 0.171 M solution of hydroiodic acid.

If 27.0 mL of base are required to neutralize 10.6 mL of the acid, what is the molarity of the calcium hydroxide solution?

_______M calcium hydroxide

An aqueous solution of hydrobromic acid is standardized by titration with a 0.162 M solution of calcium hydroxide.

If 23.9 mL of base are required to neutralize 27.6 mL of the acid, what is the molarity of the hydrobromic acid solution?

_______M hydrobromic acid

2.

A 12.2 g sample of an aqueous solution of hydroiodic acid contains an unknown amount of the acid.
If 24.1 mL of 0.305 M barium hydroxide are required to neutralize the hydroiodic acid, what is the percent by mass of hydroiodic acid in the mixture?

______% by mass

A 11.1 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid.
If 22.4 mL of 0.467 M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass of hydrobromic acid in the mixture?

______% by mass

The human body contains 0.20% natural potassium. K-40 represents 0.0117% of naturally occurring potassium. 1. What is the radioactivity due to K-40 for a person weighing 70 kg? 2. What is the radioactivity due to K-40 for all people on Erath?

by comparing the instrumental design of a spectrophotometer and the spectrofluorometer, why does the emission spectrum of the blank have well defined peaks while the absorption spectrum is nearly flat?

(hint how do you define absorbance)

What are some medical or commercial applications of gases, and how are gas laws a part of those applications? Post a thorough initial response to the discussion question (at least 7-10 sentences, or approximately 150-200 words).

What must be the molarity of an aqueous solution of NH3 if it is 4.3 % ionized? Express your answer using two significant figures.

A student makes a solution in the laboratory by dissolving 53.5 g of NH₄Cl in enough water to make 375 mL of solution, with a density of 1.05 g/mL

a. Calculate the Molarity of the solution
b. Calculate the % mass of the NH₄Cl in the solution.
c. Calculate the mole fraction of NH₄Cl in the solution
d. Calculate the molality of NH₄Cl in the solution

**Please show all work

What volume of O2 at 836 mmHg and 31 ∘C is required to synthesize 12.5 mol of NO?

Additional info: The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO)gas as shown by the unbalanced equation given here:

?NH3(g)+?O2(g)→?NO(g)+?H2O(g)

A fixed quantity of gas at 21 ∘C exhibits a pressure of 758 torr and occupies a volume of 5.42 L .

A) Calculate the volume the gas will occupy if the pressure is increased to 1.89 atm while the temperature is held constant.

B) Calculate the volume the gas will occupy if the temperature is increased to 185 ∘C while the pressure is held constant.

Part A Table of C-13 NMR data for 1-phenylcyclohexanol using the following headings for each compound (carbon types: CH, CH2, CH3, CH-OH, etc) Chemical Shift (ppm) Carbon Type

Part B Table of C-13 NMR data for 1-phenylcyclohexene using the following headings for each compound (carbon types: CH, CH2, CH3, CH-OH, etc):

Chemical Shift (ppm) Carbon Type

Give detailed explanation of the chemical Shift only and show the carbon labeled.

What are the theoretical bond energies and theoretical enthalpies for benzoic acid and sucrose?

Balance the following chemical equation:

Cu(s)+HNO3(aq)=Cu(NO3)2+NO(g)+H2O(l).

I missed this question on a quiz after trying to balance it both algebraically and by standard guess and check methods. Several classmates missed it as well. The answer is all over the internet, but what I need is a step by step explanation on how this would be balanced. Thank you!

Consider that a single solution that is listed as 1M NaCl has a total ion concentration that is twice as large due to the chemical formula containing two ions that are dissociatedin solution:

(1 mol Na⁺ ions + 1 mol Cl^- ions)/(1 L soln) = 2 mol ions/L soln = 2M ions

A. If one adds 1.0L of a 1.0M NaCl solution to 1.0L of a 1.0M NaCl solution, then what is the concentration of NaCl? What is the total ion concentration?

B. Generalize from the previous question: if one mixes any unreactive solutions that start with the same [ions], then what happens to the [ions] in the mixture?

C. Extrapolate from the previous question: if one mixes two solutions that initially have the same concentrations of ions but some of the ions react to form an insoluble solid, then what happens to the concentration of ions in the mixture?

D. Starting with a 10.00mL solution that is 0.300 M C₅H₁₀O₅, determine the concentration of sugar at four stages of mixing with a 7.00 M C₅H₁₀O₅​. Determine the concentration of sugar after a total of 0.50mL, 5.00mL, 500mL and eventually 5.000L of 7.00 M C₅H₁₀O₅​ are added. Sketch a plot of final concentration vs. volume of the 7.00M soln. Show any asymptotes with a dashed line.

E. If one mixes two unreactive solutions together, but the solutions have different concentrations, then what are the possible trends in solute concentration as one adds more and more of one solution? As more of one is added, is there an upper or lower limit? Consisder all cases.

Describe how you would prepare a liter aqueous solution of each of the following reagents
(a) 1 M glycine
(b) 0.5 M glucose
(c) 10 mM ethanol
(d) 100 mM hemoglobin

A 1.5 kg block of iron at 32 ∘C is rapidly heated by a torch such that 14 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (14 kJ ) was quickly transferred to a 890 g pellet of copper at 31 ∘C, what temperature would the copper reach before it begins losing heat to the surroundings? Use the equation for heat capacity and the following heat capacity values: qcs, Fe(s)cs, Cu(s)===mcsΔT0.450 J/(g⋅∘C)0.385 J/(g⋅∘C)