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Honda EV6010 Generator does not speed up automatically under a loaded condition. If turn on a large electrical load the generator will bog down and stall. If I manually turn up the speed and then connect the larger load it will work fine. If the load is removed the idle will of course stay up. What do i need to replace to fix this problem?

A 10.25 grams sample of metal alloy is heated to 99.10 C and then is dropped into 20.0 g of water in a calorimeter at 18.53 C. If the water temperature increases to 22.03 C, what is the specific heat capacity of the alloy? The specific heat capacity for water is 4.184 J/ gC.

Consider the combustion of carbon monoxide (CO) in oxygen gas:

2CO(g) + O2(g) --> 2CO2(g)

Starting with 3.60 moles of CO, calculate the number of moles of CO2 produced if there is enough oxygen gas to react with all of the CO.

Over time, MgO (s) can absorb water. If your MgO sample was hydrated, would this effect your data? Would the (change in H) determined be more or less negative?

Mg +2 HCl → MgCl2 + H2 -467 kJ/mol

MgCl2 +H2O → MgO + 2 HCl -151 kJ/mol

H2 + ½O2 → H2O -286 kJ/mol

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Mg + ½O2 → MgO

calculate the heat of the reaction, change in H, from the following data.

MgO (s) + 2 H+ (aq) → Mg2+(aq) + H2O (l)

Hf ° (KJ/g mol)

MgO (s) -602

H+ (aq) 0

H2O (l) -286

Mg2+ (aq) -467

What is the balanced net ionic reaction of magnesium oxide reacting with aqueous hydrochloric acid to produce aqueous magnesium chloride and water.

Calculate using the change in H for this reaction from the following heats of formation.

Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g)

change in Hf ° (KJ/g mol)

Mg (s) 0

H+ (aq) 0

Mg2+ (aq) -467

Given the following data:

Cu2 (s) + ½O2 (g) → 2 CuO (s) change in H° = -144 kJ

Cu2 (s) → Cu (s) + CuO (s) change in H° = +11 kJ

Calculate the standard enthalpy of formation, change in Hfinal ° of CuO (s). Hint: Look up the definition of standard enthalpy of formation then write the reaction for the standard enthalpy of formation of CuO (s).

Using the change in H final ° values given, calculate change in H final ° for the combustion of carbon disulfide.

CS2 (l) + 3 O2 (g) → CO2 (g) + 2 SO2 (g)

Hf ° (KJ/g mol)

CS2 (l) 89.7

CO2 (g) -393.5

SO2 (g) -297.0

3. When I did this experiment I found that the heat of reaction, measured for MgO reacting with HCl, increased with increasing HCl concentration. The heat released in this reaction was significantly higher with 6.0 M HCl was used than when 2.0 M HCl was used. The heat released using 6.0 M was in better agreement with the actual value. Explain why this effect may be observed.

In a Thermo Chemistry experiment, if the hot metal sample was wet, before it was transferred to the water in the calorimeter, how would this affect the experimental heat capacity of the metal? Explain your answer in terms of the specific heat of water relative to that of tin which is the metal used in this experiment.

The heat of combustion for a sample of coal is 23.0 °C KJ/g. What quantity of coal in grams must be burned to heat 500.0 g of water from 20.0 °C to 95.0 °C. The specific heat capacity of water is 4.184 J-1 °C-1 g.

Consider the following reaction.

H2 (g) + 2 CO (g) → H2O2 (I) + 2 C (s) Change of H = +33.3 kJ

Calculate the enthalpy changes when 5 mole of CO is consumed.

The combustion of carbon monoxide is exothermic.

CO (g) + ½O2 (g) → CO2 (g) Change of H = -283.0 kJ

Determine change of H for each of the following reactions.

a) 2 CO (g) + O2 (g) → 2 CO2 (g)

b) 2 CO2 (g) → 2 CO2 (g) + O2 (g)

A 10.0 g piece of metal at 100 °C is transferred to a calorimeter containing 50.0 mL of water initially at is 25.0 °C. Calculate the specific heat capacity of the metal if the heat the heat capacity of the calorimeter Ccal is 25.0 J/°K. The final temperature, Tfinal is 25.6 °C.

If 0.49 g of a gas occupies 275 mL at 26 °C and 1.10 atm, calculate the molar mass of the gas.

Explain the function of FeCL3 in the decomposition of H2O2? If we used 5.0 mL of 3 M FeCl3 rater than 4.5 mL of 3 M FeCl3, would it have made any difference in the amount of oxygen gas collected? Explain why or why not.