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The answer to this question will depend on what the substance that is reacting is. You will need to find the appropriate standard enthalpy value, which corresponds to the amount of enthalpy change when one mole of matter is transformed by a chemical reaction in standard conditions.
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How much energy is absorbed when 356 g of ethanol 46.0 g molboils The heat of vaporization of ethanol is 38.6 kJ mol?
To calculate the energy absorbed, first convert the mass of ethanol from grams to moles. 356 g of ethanol is 356/46.0 = 7.74 moles. Then, multiply the moles of ethanol by the heat of vaporization: 7.74 mol * 38.6 kJ/mol = 298.56 kJ of energy absorbed.
How much heat is absorbed when 75 g of liquid carbon tetrachloride (CCl4) vaporizes into a gas?
The heat absorbed during vaporization is called the heat of vaporization. For carbon tetrachloride, the heat of vaporization is 30.5 kJ/mol. To calculate the heat absorbed when 75 g of CCl4 vaporizes, you would first convert grams to moles using the molar mass of CCl4. Then, use the heat of vaporization to calculate the total heat absorbed.
When 10 g of diethyl ether is converted to vapor at its boiling point about how much heat is absorbed (C4H10O and Icirc and 148Hvap 15.7 kJmol boiling point 34.6 and Acirc and degC)?
The molar mass of diethyl ether (C4H10O) is 74.12 g/mol. Therefore, 10 g of diethyl ether is approximately 0.135 moles. The heat absorbed to convert this amount of diethyl ether from liquid to vapor at its boiling point is given as 15.7 kJ/mol. So, for 0.135 moles, approximately 2.12 kJ of heat is absorbed.
How much heat is absorbed if 2.60mol of A reacts if heat of formation in -237kJmol?
You must first convert kJ/mol. So.. -237kJ x (1kJ / 2.60mol) = -91.15kJ You then must take this and multiple by (-1), since you cannot have a negative heat. (-91.15kJ x -1) = 91.15kJ
When 30 grams of water is converted into steam how much heat is absorbed?
q = mHvq = heatm = mass (30g)Hv = heat of vaporization (2,260J/g)q = (30g)(2,260J/g)q = 67,800JWhen 30 grams of water is converted into steam, how much heat is absorbed?67,800J of heat, also represented as 67.8kJ of heat is absorbed.
How much energy is absorbed when 356 g of ethanol 46.0 g molboils The heat of vaporization of ethanol is 38.6 kJ mol?
To calculate the energy absorbed, first convert the mass of ethanol from grams to moles. 356 g of ethanol is 356/46.0 = 7.74 moles. Then, multiply the moles of ethanol by the heat of vaporization: 7.74 mol * 38.6 kJ/mol = 298.56 kJ of energy absorbed.
How much heat is absorbed when 75 g of liquid carbon tetrachloride (CCl4) vaporizes into a gas?
The heat absorbed during vaporization is called the heat of vaporization. For carbon tetrachloride, the heat of vaporization is 30.5 kJ/mol. To calculate the heat absorbed when 75 g of CCl4 vaporizes, you would first convert grams to moles using the molar mass of CCl4. Then, use the heat of vaporization to calculate the total heat absorbed.
How much energy is absorbed when 23.1 moles of water vaporize?
540 calories per gram is absorbed when water vaporizes at its boiling point. Called the latent heat of vaporization. 540 x 23.1 x 18 = 224532 calories
When 10 g of diethyl ether is converted to vapor at its boiling point about how much heat is absorbed (C4H10O and Icirc and 148Hvap 15.7 kJmol boiling point 34.6 and Acirc and degC)?
The molar mass of diethyl ether (C4H10O) is 74.12 g/mol. Therefore, 10 g of diethyl ether is approximately 0.135 moles. The heat absorbed to convert this amount of diethyl ether from liquid to vapor at its boiling point is given as 15.7 kJ/mol. So, for 0.135 moles, approximately 2.12 kJ of heat is absorbed.
How much heat is absorbed by land and sea?
51%
How much heat must be absorbed by 50 grams?
Joule (J) is a unit of energy.Gram (g) is a unit for mass.
How much heat is absorbed if 2.60mol of A reacts if heat of formation in -237kJmol?
You must first convert kJ/mol. So.. -237kJ x (1kJ / 2.60mol) = -91.15kJ You then must take this and multiple by (-1), since you cannot have a negative heat. (-91.15kJ x -1) = 91.15kJ
How much heat is absorbed when 52.3 g H2O(l) at 100 and degC and 101.3 kPa is converted to steam at 100 and degC (The molar heat of vaporization of water is 40.7 kJmol.)?
To calculate the heat absorbed when converting 52.3 g of water to steam at 100 °C, we first convert the mass of water to moles using the molar mass of water (approximately 18.02 g/mol). The number of moles is ( \frac{52.3 , \text{g}}{18.02 , \text{g/mol}} \approx 2.90 , \text{mol} ). The heat absorbed can then be calculated using the molar heat of vaporization: ( q = n \times \Delta H_{vap} = 2.90 , \text{mol} \times 40.7 , \text{kJ/mol} \approx 118.0 , \text{kJ} ). Thus, approximately 118.0 kJ of heat is absorbed.
When 30 grams of water is converted into steam how much heat is absorbed?
q = mHvq = heatm = mass (30g)Hv = heat of vaporization (2,260J/g)q = (30g)(2,260J/g)q = 67,800JWhen 30 grams of water is converted into steam, how much heat is absorbed?67,800J of heat, also represented as 67.8kJ of heat is absorbed.
How much heat exactly is absorbed by the ozone or what temperature would the earth be if there was no ozone?
23 percent of incoming solar energy is usually absorbed by the ozone. Temperature, not how much
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
What mass of needed to generate kj heat when reacting?
To determine the mass needed to generate a specific amount of heat (in kJ) during a reaction, you need to know the enthalpy change (ΔH) of the reaction, which indicates how much heat is absorbed or released per mole of reactant. Using the formula ( q = n \times ΔH ), where ( q ) is the heat in kJ and ( n ) is the number of moles, you can rearrange this to find ( n = \frac{q}{ΔH} ). Then, multiply the number of moles by the molar mass of the reactant to obtain the required mass.
