Which of the following mixture types is characterized by the settling of particles?a. solution
b. suspension
c. colloid
d. hydrate

Answer:

The Carnot engine operates based on the principles of the Carnot cycle, which is a theoretical idealized thermodynamic cycle. To calculate the work done by the engine, we need to use the formula for the efficiency of the Carnot cycle.

The efficiency of a Carnot engine is given by the equation:

Efficiency = 1 - (T2 / T1),

where T2 is the exhaust temperature in Kelvin and T1 is the burn temperature in Kelvin.

First, we need to convert the temperatures from Celsius to Kelvin.

The burn temperature is 1957 ˚C, so we add 273 to convert it to Kelvin:

T1 = 1957 + 273 = 2230 K.

The exhaust temperature is 500 ˚C, so we add 273 to convert it to Kelvin:

T2 = 500 + 273 = 773 K.

Now we can calculate the efficiency:

Efficiency = 1 - (T2 / T1) = 1 - (773 / 2230).

Next, we need to calculate the heat input, which is the energy released by burning 1 kg of methane.

The energy released by burning methane can be calculated using the heat of combustion of methane, which is -891 kJ/mol.

To convert this to joules per kilogram, we need to know the molar mass of methane, which is 16 g/mol.

1 kg of methane is equal to 1000 g, so the number of moles of methane in 1 kg is:

1000 g / 16 g/mol = 62.5 mol.

The heat released by burning 1 kg of methane is:

-891 kJ/mol * 62.5 mol = -55,687.5 kJ.

To convert this to joules, we multiply by 1000:

-55,687.5 kJ * 1000 = -55,687,500 J.

Now we can calculate the work done by the engine:

Work = Efficiency * Heat input.

Substituting the values we calculated:

Work = (1 - (773 / 2230)) * (-55,687,500 J).

Finally, we can calculate the work done by the engine in joules.

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The combustion reaction of the unknown compound can be written as follows:

Other part of the question is discussed below:

We know that 3.50 g of the compound produced 5.13 g of carbon dioxide and 2.10 g of water. This means that 1.63 g of oxygen were also produced in the reaction.

The mass of oxygen in the original sample is equal to the mass of oxygen produced in the reaction, so the original sample contained 1.63 g of oxygen.

The total mass of carbon and hydrogen in the original sample is equal to the mass of the sample minus the mass of oxygen, which is 3.50 g - 1.63 g = 1.87 g.

We can find the number of moles of hydrogen in the original sample by dividing the mass of hydrogen by the molar mass of hydrogen (1.008 g/mol). This gives us 1.87 g / 1.008 g/mol = 1.86 moles of hydrogen.

Therefore, the answer is 1.86

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Final answer:

By dividing the mass of water produced in combustion by the molar mass of Hydrogen in water, we find that the original compound contained 1.05 mol of Hydrogen.

Explanation:

To determine the mole amount of Hydrogen in the compound, you have to consider the reaction applied, and how it applies to the law of conservation of mass. Combustion of the compound produces carbon dioxide (CO2) and water (H2O). For water, one mol equals to the molar mass of H which is 1 g/mol, times the amount of H in water which is 2 to get 2 g/mol. Now knowing that 2.10 g of water were produced from combustion, we divide this by the molar mass of H-in-water to get the number of hydrogen moles in the original sample. So, the calculation will be 2.10 g/ 2 (g/mol) = 1.05 mol. So, the original compound contained 1.05 mol of hydrogen.

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Answer:

1-There Must be some displacement in the direction of force.                                                  2-Angle between force and displacement is 0°.