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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Which statement is true about this reaction?
(1) Each Al loses 2e- and each Cu2+ gains 3e-
(2) Each Al loses 3e- and each Cu2+ gains 2e-
(3) Each Al3+ gains 2e- and each Cu loses 3e-
(4) Each Al3+ gains 3e- and each Cu loses 2e-
b. ionic bonding
c. metallic bonding
d. nonpolar covalent bonding
e. polar covalent
B. Jupiter
C. Mars
D. Neptune
Answer: Jupiter is believed to have prevented the asteroids in the asteroid belt from forming a planet.
a. mass number: 24, charge: +2
b. mass number: 22, charge: neutral
c. mass number: 34, charge: -2
d. mass number: 34, charge: +2
The mass mass number is 22 and the charge of the atom is +2. The correct answer is option A
1. The mass number of the atom can be obtained as follow:
Mass number = number of proton + number of neutron
= 12 + 12
= 24
2. The charge of the atom can be obtained as follow:
Charge = number of protons - number of electrons
= 12 - 10
= +2
Thus, the mass number is 24 and the charge is +2. The correct answer to the question is option A
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Answer:
when 1.00 g of magnesium reacts with 5.00 g of bromine, approximately 7.57 g of magnesium bromide is formed.
Explanation:
To find the mass of magnesium bromide formed when 1.00 g of magnesium reacts with 5.00 g of bromine, you need to first write a balanced chemical equation for the reaction between magnesium and bromine. The balanced equation for the formation of magnesium bromide (MgBr2) is as follows:
Mg + Br2 → MgBr2
Now, you can calculate the molar mass of each substance involved in the reaction:
Molar mass of Mg (magnesium) = 24.31 g/mol
Molar mass of Br2 (bromine) = 2 * 79.90 g/mol = 159.80 g/mol
Molar mass of MgBr2 (magnesium bromide) = 24.31 g/mol + 2 * 79.90 g/mol = 184.11 g/mol
Next, calculate the number of moles for each reactant:
Moles of Mg = Mass (1.00 g) / Molar mass (24.31 g/mol) = 0.0411 moles
Moles of Br2 = Mass (5.00 g) / Molar mass (159.80 g/mol) = 0.0313 moles (approximately, rounded to four decimal places)
Now, determine the limiting reactant. To do this, compare the mole ratio between Mg and Br2 in the balanced equation. The balanced equation shows that 1 mole of Mg reacts with 1 mole of Br2. Therefore, the limiting reactant is the one that is present in the smaller amount relative to the balanced equation's stoichiometry.
In this case, magnesium (0.0411 moles) is present in a smaller amount than bromine (0.0313 moles). So, magnesium is the limiting reactant.
Now that you know magnesium is the limiting reactant, you can calculate the mass of magnesium bromide formed using the stoichiometry of the balanced equation. According to the balanced equation, 1 mole of Mg produces 1 mole of MgBr2.
Moles of MgBr2 formed = Moles of Mg (limiting reactant) = 0.0411 moles
Now, calculate the mass of magnesium bromide formed:
Mass of MgBr2 = Moles of MgBr2 × Molar mass of MgBr2
Mass of MgBr2 = 0.0411 moles × 184.11 g/mol = 7.57 g
So, when 1.00 g of magnesium reacts with 5.00 g of bromine, approximately 7.57 g of magnesium bromide is formed.
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