Reference no: EM132650795
Write a equilibrium constant expression for the reversible reaction. Remember to use brackets, [], for concentrations, and use exponents where needed.
2SO3(g)?O2(g) + 2SO2(g)
A 5.18-g sample of octane is burned in a bomb calorimeter containing 2.43 × 102 g H2O. Given that 1.30 × 103 cal of energy is released if the water temperature increases 5.36°C. Calculate the energy released in J.
Write the equilibrium constant expression for the following reaction. Remember to use brackets, [ ], for concentrations and use exponents where needed. Click in the answer box to activate the palette.
N2(g) + 3H2(g) ? 2NH3(g)
Write the equilibrium constant expression for the following reaction. Remember to use brackets, [ ], for concentrations and use exponents where needed, but do not show physical states in your answer. Click in the answer box to activate the palette.
C(s) + H2O(g) ? CO(g) + H2(g)
If 0.10 mol ammonium chloride (NH4Cl) is dissolved in water producing 2.00 × 102 g of solution, the water temperature decreases from 24.2°C to 18.6°C. If the specific heat of the solution is 1.00cal/g-°C, calculate the quantity of energy involved in the process.
N2(g) + 2O2(g)? 2NO2(g) calculate the equilibrium constant.
A 1.0-g sample of a candy bar (which contains lots of sugar and fats!) was burned in a bomb calorimeter. A 3.8°C temperature increase was observed for 1.00 × 103 g of water. The entire candy bar weighed 3.0 ounces (oz). Calculate the fuel value (in Cal) of the sample.