Kerosene, a common space-heater fuel, is a mixture of hydrocarbons whose "average" formula is C12H26.

Write a balanced equation, using the simplest whole-number coefficients, for the complete combustion of kerosene to gases.

Silver bromide is used to coat ordinary black-and-white photographic film, while high-speed film uses silver iodide. (a) When 50.0 mL of 5.0 g/L AgNO3 is added to a coffee-cup calorimeter containing 50.0 mL of 5.0 g/L Nal, with both solutions at $25 ^ { \circ } \mathrm { C }$ what mass of Agl forms? (b) find $\Delta H _ { \mathrm { rxn } } ^ { \circ }$ (c) What is $\Delta$ Tsoln (assume the volumes are additive and the solution has the density and specific heat capacity of water)?

A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(ll) oxide: $2 \mathrm { HgO } ( \mathrm { s } ) \rightarrow 2 \mathrm { Hg } ( \mathrm { l } ) + \mathrm { O } 2 ( \mathrm { g } ) \Delta \mathrm { H } \mathrm { rxn } = 181.6 \mathrm { kJ }$ (a) How much heat is needed to decompose 555 g of the oxide? (b) If 275 kJ of heat is absorbed, how many grams of Hg form?

A grating has exactly 8000 slits uniformly spaced over 2.54 cm and is illuminated by light from a mercury vapor discharge lamp. What is the expected angle for the third-order maximum of the green line ($\lambda = 546 \mathrm { nm }$)?

Kerosene, a common space-heater fuel, is a mixture of hydrocarbons whose "average" formula is $\mathrm{C}_{12} \mathrm{H}_{26}$.
(c) Calculate the heat produced by combustion of $0.50 \mathrm{gal}$ of kerosene $(d$ of kerosene $=0.749 \mathrm{~g} / \mathrm{mL})$.

Determine whether each argument is valid or invalid. All A are B, no C are B, and all D are C. Thus , no A are D.

One mole of nitrogen gas confined within a cylinder by a piston is heated from $0 ^ { \circ } \mathrm { C }$ to $819 ^ { \circ } \mathrm { C }$ at 1.00 atm. (a) Calculate the work of expansion of the gas in joules $( 1 J = 9.87 \times 10 - 3 \ atm \cdot L)$ . Assume all the energy is used to do work. (b) What would be the temperature change if the gas were heated with the same amount of energy in a container of fixed volume? (Assume the specific heat capacity of N2 is 1.00 J/g $\cdot K)$.

Liquid methanol (CH3OH) can be used as an alternative fuel in pickup and SUV engines. An industrial method for preparing it uses the catalytic hydrogenation of carbon monoxide: $\mathrm { CO } ( g ) + 2 \mathrm { H } _ { 2 } ( g ) \stackrel { \mathrm { calalyst } } { \longrightarrow } \mathrm { CH } _ { 3 } \mathrm { OH } ( l )$ How much heat (in kJ) is released when 15.0 L of CO $85 ^ { \circ } \mathrm { C }$ and 112 kPa reacts with 18.5 L of H2 at $75 ^ { \circ } \mathrm { C }$ and 744 torr?

Copper(l) oxide can be oxidized to copper(ll) oxide: $\mathrm { Cu } _ { 2 } \mathrm { O } ( s ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( g ) \longrightarrow 2 \mathrm { CuO } ( s ) \quad \Delta H _ { \mathrm { rxn } } ^ { \circ } = - 146.0 \mathrm { kJ }$ Given $\Delta H _ { \mathrm { f } } ^ { \circ }$ of $\mathrm { Cu } _ { 2 } \mathrm { O } ( s ) = - 168.6 \mathrm { kJ } / \mathrm { mol }$, find $\Delta H _ { f } ^ { \circ }$ of $\mathrm { CuO } ( s )$

Calculate $\Delta H _ { \mathrm { rxn } } ^ { \circ }$ for each of the following: (a) $SiO2(s) + 4HF(g) \rightarrow SiF4(g) + 2H2O(l)$ (b) $C2H6(g) + O2(g) \rightarrow CO2(g) + H2O(g)$ [unbalanced]

Acetylene burns in air according to the following equation: $\mathrm { C } _ { 2 } \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 5 } { 2 } \mathrm { O } _ { 2 } ( g ) \longrightarrow 2 \mathrm { CO } _ { 2 } ( g ) + \mathrm { H } _ { 2 } \mathrm { O } ( g ) \ \Delta H _ { \mathrm { rxn } } ^ { \circ } = - 1255.8 \mathrm { kJ }$ Given $\Delta H _ { \mathrm { f } } ^ { \circ }$ of CO2(g) = -395.5 kJ/mol, find $\Delta H _ { \mathrm { f } } ^ { \circ }$ of H2O(g) = ?241.8 kJ/mol, find $\Delta H _ { \mathrm { f } } ^ { \circ }$ of C2H2(g).

Comprehensive Problems. Stearic acid $(C _ { 18 }H _ { 36 } O _ { 2 } )$ is a fatty acid, a molecule with a long hydrocarbon chain and an organic acid group (COOH) at the end. It is used to make cosmetics, ointments, soaps, and candles and is found in animal tissue as part of many saturated fats. In fact, when you eat meat, you are ingesting some fats containing stearic acid. (a) Write a balanced equation for the combustion of stearic acid to gaseous products. (b) Calculate $\Delta H _ { \mathrm { rxn } } ^ { \circ }$ (c) Calculate the heat ( q ) released in kJ and kcal when 1.00 g of stearic acid is burned completely. (d) A candy bar contains 11.0 g of fat and 100. Cal from fat; is this consistent with your answer for part (c)?

When steam is passed over iron filings, solid iron(III) oxide and gaseous hydrogen are produced in a reversible reaction. Write the balanced chemical equation and the equilibrium constant expression for the reaction, which yields iron(III) oxide and hydrogen gas.

Which organelle plays an important role in cell division?