3. CH3OH is synthesized via the following reaction: CO (g) + 2H2 (g)  CH3OH (g) . If the reaction occurs at 748 mmHg and 25 °C , what volume of H2 gas (in L) is necessary to synthesize 25.8 g CH3OH? What volume (L) of CO gas is required?

4. Hydrogen gas can be formed by the reaction of methane and water according to the following equation: CH4 (g) + H2O (g)  CO (g) + 3H2 (g) . In one reaction, 25.5 L of methane gas (at P = 732 Torr, T = 25 °C) is mixed with 22.8 L of water vapor (at P = 702 Torr, T = 125 °C). The reaction produces 26.2 L hydrogen gas at STP. What is the percent yield of the reaction?

Describe two chemical reactions that you encounter on a regular basis.

Figure P30.23 is a cross-sectional view of a coaxial cable. The center conductor is surrounded by a rubber layer, which is surrounded by an outer conductor, which is surrounded by another rubber layer. In a particular application, the current in the inner conductor is I₁ = 1.10 A out of the monitor, and the current in the outer conductor is I₂ = 2.84 A into the monitor. Determine the magnitude and direction of the magnetic field at point a.

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH.

A solution is made by titrating 8.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH?

More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 46.0 mL ?

No idea how to do this! Please explain..thanks!

A ground state hydrogen atom absorbs a photon of λ = 94.91 nm, exciting the electron to a higher energy (quantum) level. The electron then decays to a lower, intermediate energy level, emitting a photon of λ = 1281 nm. From that intermediate energy level the electron decays back to the ground state, emitting another photon. a) What is the highest energy level attained by the electron?

b) What was the intermediate energy level of the electron?

c) What was the λ of the second photon?

Calculate the pH of the buffer formed by mixing equal volumes [C₂H₅NH₂]= 1.68M with [HClO₄]= 0.984M . Kb=4.3

Design a separation scheme for Cu2+, Fe3+, Mn2+, and Ni2+ include equations for all reactions.

The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10^ -6 mol/L when about a tenth of a mole of the acid os dissolved in a liter of water.

                          * Weak or Strong?           *Species present at 10^ -6 mol/L or greater when dissolved in water.

HBrO3

H2SO3

HClO2

HBr

Calculate the concentrations for all components of the following reaction at equilibrium:

PCl3 + Cl2 ⇄ PCl5

Equilibrium constant K=16

Initial concentration PCl5 = 0.5 M

why is substitution of a proline amino acid in the middle of an alpha-helix always disruptive?

Calculate the molar solubility of BaSO₄ in a solution containing 0.70M SO₄^2- ion.

_________ x 10 ^_______

Consider the reaction that converts pyruvic acid (CH3COCOOH) into gaseous acetaldehyde (CH3CHO) and gaseous CO2, which is catalyzed in aqueous solution by the enzyme pyruvate decarboxylase. Assume ideal gas behavior for CO2.

(a) Calculate delta-G (298 K) for this reaction at 160 bar.

(b) Calculate delta-G (298K) for this reaction at 100 bar. State any important assumption needed in addition to ideal gas behavior.

Pure solid NaH2PO4 is dissolved in distilled water, making 100.00 ml of solution. 10.00ml of this solution is diluted to 100.00 ml to prepare the original phosphate standard solution. Three working standard solutions are made from this by pipetting 0.8ml, 1.5ml and 3.0 ml of the original standard solution into 100.00 ml volumetric flasks. Acid and molybdate reagent are added and the solutions are diluted to 100.00 ml. You may assume that all these absorbance measurements have already been corrected for any blank absorbance. The absorbance of each is measured in the spectrophotometer. Mass of NaH2PO4 (mg) 512.2 Absorbance Standard 1 (0.8 ml) 0.1922 Standard 2 (1.5 ml) 0.3604 Standard 3 (3.0 ml) 0.7209 Calculate the following Concentration of original phosphate standard (mM) , Concentration of Standard 1(mM), Concentration of Standard 2(mM), Concentration of Standard 3(mM), Slope of calibration line?

Question 3

Sodium nitrite (NaNO₂) is a commonly used meat preservative.

a. Knowing that the K_a of nitrous acid (HNO₂) is 4.5 x 10^-4 M, calculate the pH of a 0.25 M sodium nitrite (NaNO₂) solution.

b. How many grams of sodium nitrite (NaNO₂) must be added to 100.0 mL of 0.150 M nitrous acid (HNO₂) to make a buffer solution with a pH of 3.50?

c. If 0.05 g of NaOH (s) are added to 100.0 ml of the buffer solution prepared in part (b), what is the new pH?

Use vibrational transitions and energy stored in the sulfur dioxide molecule to explain climate change