Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) 2 NH3(9) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O₂(g) → HNO3(g) + H₂O(g) ΔΗ= - 330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. AH=-92. kJ

The reaction below is a  exothermic or endothermic reaction. 2SO3(g) + Heat ⇋ 2SO2(g) + O2(g)

4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).

The reaction below has an enthalpy change of 198 kJ. How many grams of sulfur dioxide are produced when 564 kJ is absorbed?   2 SO3 (g) →  2 SO2 (g)  +  O2 (g)

The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol

Which chemical reaction below yields the heat of formation of liquid ammonia (NH3)? 3H(g) + N(g) →→→ NH3(e) H₂ (g) + N2₂ (g)→→ NH3(e) 3/2 H₂ (g) + 1/2 N₂ (g)→ NH3 (e) 3H₂(g) + N₂ (g)→ 2NH3(e) 3/2 H₂(g) + N(g)→ NH3(e)

33 of 35 > Macmillan Learning When methanol, CH3OH, is burned in the presence of oxygen gas, O₂, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH₂OH(g) + O₂(g) → CO₂(g) + 2 H₂O(1) ΔΗ = −764 kJ How much methanol, in grams, must be burned to produce 601 kJ of heat? mass:

What is the kinetic energy of a 4.15x10 kilogram golf ball moving at a velocity of 44.3 meters per second? (KE =½m v) Joules

Humans are heterotrophs that consume food for energy. These foods comprise of sugars that are broken down by enzymic activity within the body for producing energy. This process, called cellular respiration, occurs according to the chemical equation: C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1 a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of theequilibrium constant (Kc) and predict the whether the products or reactants will befavoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are[CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reactionquotient (Qc). Compare the Kc and Qc values and predict the favoured direction of thereaction.d) Explain the effect on equilibrium ofi) Increasing temperatureii) Increasing…