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)

What are the changes in enthalpy, entropy, and free energy for the hydrogenation of C2H4 to C2H6, and C3H6 to C3H8 at 25 degrees C.

1. The molecular weight between crosslinks (MC) is one of the most important parameter that describes the thermoset network structure. Describe how the MC is related to the following properties:(a) T_g, (b) modulus, (c) elongation to break, and (d) solvent resistance. How do you measure MC value?

A zero order reaction starts with an initial concentration of reactant of 1.00 M and has a rate constant of 1.65x10^-5M/s. What is the concentration of the reactant after 100 seconds?

You have 525 mL of an 0.15 M acetic acid solution. What volume (V) of 2.00 M NaOH solution must you add in order to prepare an acetate buffer of pH = 5.32? (The pKa of acetic acid is 4.76.)

I'm trying to under stand the Haber process and this equilibrium reaction N2 +3H2 -----> 2NH3 + energy. In order to increase the yields of ammonia

1. remove amonia as it is formed

2. add an inhibitor

3. heat the reaction vessel

4. decrease the pressure in the reaction vessel.

5) Zn1+xO, Ti1+xO, Cu2S1+x, CuI1+x and ZnO1+x are semiconductors. What type of semiconductors are they (n- or p-type)?

One of the possible initial steps in the formation of acid rain is the oxidation of the pollutant SO2 to SO3 by the following reaction: SO2(g) + 1/2 O2(g) -> SO3(g) The reaction is exothermic, meaning that it is spontaneous at lower temperatures, but becomes nonspontaneous at higher temperatures. At what temperature does it change from being spontaneous to nonspontaneous?

Molecule ΔHf (kJ/mol) @ 25°C S (J/molK) @ 25°C

SO2(g) -296.8 248.2  

SO3(g) -395.7 256.8

503 K

1052 K

98.7 K

99.1 K

Consider the titration of 100.0 mL of 0.130 M H₂NNH₂ (K_b= 3.0 x 10^-6) by 0.260 M HNO₃. Calculate the pH of the resulting solution after the following volumes of  have been added: 0.0 mL, 20.0 mL, 40 mL, 50 mL, 100 mL.

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate in 200 ml of 1M acetic acid? The Ka for acetic acid id 1.7*10^-5.

B. Calculate the pH of the solution if 10 ml of 0.100M HCl is added to the solution.

C. What will the pH be if 5.00 ml of 0.150M NaOH was added to solution in B?

D. Write the equation when an acid and a base are added to the buffer system.

Consider the system:

A (aq) → B (aq)

at 251 K where ΔG^oform A = -11.7 kJ/mol and ΔG^oform B = -14.1 kJ/mol. Calculate the concentration of A at equilibrium when 1.71 mol of A and 1.35 mol of B are mixed in water to form exactly one liter of solution.