I hold a BS in Chemistry, a Master of Arts degree in Teaching, and a second Master of Arts degree in Educational Leadership. I have been teaching for 12 years. I have taught all levels of chemistry (college prep, honors, AP, advanced, remedial). I have also taught various levels of biology, physics, and environmental science.
Find the $x$- and $y$-intercepts (if they exist). Then graph the line.$x-3 y=6$
Find the $x$- and $y$-intercepts (if they exist). Then graph the line.$x-5=2$
Hess's LawThe enthalpy changes for the following reactions can be measured:$\mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$$$\Delta_{r} H^{\circ}=-802.4 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn}$$$\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})+3 / 2 \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$$\Delta_{1} H^{\circ}=-676 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn}$(a) Use these values and Hess's law to determine the enthalpy change for the reaction $\mathrm{CH}_{4}(\mathrm{g})+1 / 2 \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$(b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.
The enthalpy changes of the following reactions can be measured:$\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$$$\Delta_{i} H^{\circ}=-1411.1 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn}$$$\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\ell)$$\Delta, H^{\circ}=-1367.5 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn}$(a) Use these values and Hess's law to determine the enthalpy change for the reaction $\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)$(b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.
These questions are not designated as to type or location in the chapter. They may combine several concepts.The following terms are used extensively in thermodynamics. Define each and give an example.(a) exothermic and endothermic(b) system and surroundings(c) specific heat capacity(d) state function(e) standard state(f) enthalpy change, $\Delta H$(g) standard enthalpy of formation
Write a balanced equation for the dissociation of each of thefollowing strong electrolytes in water:a. KCl b. CaCl2c. K3PO4 d. Fe(NO3)3
4.25 g of a certain allotrope of phosphorous, P4,reacts with 7.00 g oxygen gas to produceP4O10. P4 + 5O2 ->P4O10Which reactant will be left over after the reaction is completeand how much of it will be left over?
Given the unbalanced equation: CH4(g) + O2(g) → CO2(g) + H2O(g)16.0g of methane reacts with excess oxygen and 22.0g of carbon dioxide was collected. What is the percent yield of carbon dioxide?
0.112 M KOH solution was used to titrate a 33.00 mL sample of aweak acid solution, HC3H5O2, ofunknown concentration. 44.04 mL of base was added to reach theequivalence point. Calculate the original concentration of the acidin molarity.0.112 M 0.149 M none of the answers are correct. 0.00493 M 0.000112 M
How many grams of iron (II) oxide are produced when 9.6 g ofiron reacts with 4.5 g oxygen to produce iron (II) oxide?
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K?2 NO2 (g) ⇌ N2O4 (g)The conditions for this reaction are:P(NO2) = 0.66 barP(N2O4) = 1.5 barYou will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation).Please use the method of Gibbs energy of formation to calculate ΔrG° if needed.For partial credit, enter the value of "Q" for this reaction.
