Other Chemistry Answers

The following reaction is exothermic:
CO(g) + 2 H2(g)CH3OH(g)

How will the amount of CH3OH(g) present at equilibrium be affected by:

adding additional CO(g)?
increasing the volume of the container?
adding a catalyst to the system?
removing CO(g)?

The equilibrium constant for the following reaction is 2.84 x 10-2 at 430 oC.
2 HI(g)H2(g) + I2(g)

A lab technician places 0.200 mol of hydrogen iodide in a 1.00 L reaction vessel and allows to reach equilibrium, use an I.C.E. table to determine the equilibrium concentrations of all species.

The following reaction is at equilibrium at 500 oC
CH4(g) + H2O(g)CO(g) + 3 H2(g)

Equilibrium concentrations were found to be:

[CH4(g)] = 2.46 x 10-3 M
[H2O(g)] = 4.97 x 10-3 M
[CO(g)] = 4.55 x 10-3 M
[H2(g)] = 2.20 x 10-3 M

Calculate the equilibrium constant for this reaction.

Write the equilibrium law expression for the following reaction in terms of its molar concentrations:
SOCl2(g) + H2O(g)SO2(g) + 2 HCl(g)

Using standard enthalpies of formation, determine the ΔHreaction for the following equations:

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

Standard Enthalpies of Formation

Compound ΔHf (kJ/mol)
CO(g) -110.5
CO2(g) -393.5
CH3OH(l) -238.4
H2O(g) -241.8

Use Hess' Law to calculate enthalpy of reaction for the following equation:

2 N2(g) + 5 O2(g) → 2 N2O5(g)

Given:

2 H2(g) + O2(g) → 2 H2O(l) ΔH = -571.6 kJ /mol

N2O5(g) + H2O(l) → 2 HNO3(l) ΔH = -76.6 kJ /mol

1/2 N2(g) + 3/2 O2(g) + 1/2 H2(g) → HNO3(l)
ΔH = -174.1 kJ /mol

(Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)

Iron is made from a reaction of iron oxide with carbon monoxide in the following reaction:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

Using Hess' Law, calculate the enthalpy of reaction given:

C(s) + O2(g) → CO2(g)
ΔH = -393.5 kJ /mol

2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH = -824.2 kJ /mol

C(s) + 1/2 O2(g) → CO(g) ΔH = -110.5 kJ /mol

(Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)

250 mL of water is heated from 3 oC to 90 oC on a butane stove. Assume all the heat from combustion is used to warm the water.
C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l)

Standard Enthalpies of Formation (ΔHof):

C4H10(g) = -124.8 kJ /mol
CO2(g) = -393.5 kJ /mol
H2O(l) = -285.8 kJ /mol
a) What is the total amount of heat required for the process?

b) What is the molar heat of combustion for butane?

c) What is the mass of butane needed for this process?

(Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)

6.40 kJ of energy is needed to raise the temperature of a calorimeter and its contents 1.00 oC. When 2.00 g of propyne (C3H4(g)) is burned in a calorimeter, the temperature of the calorimeter was raised 15.0 oC. What is the molar heat of combustion of propyne?

(Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)

A sample of methanol (CH3OH(aq)), with a specific heat of 2.51 J/goC needed 27.1 kJ of energy to heat it from 22.0 oC to 52.0 oC. What is the mass of methanol used?

(Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)