Solved Question 3 4 Pts Calculate The Total Energy Required Chegg Calculate the molar heat of vaporization of ethanol using its given molecular weight. determine the amount of energy (in kj) required to vaporize 259 g of ethanol (ch3ch2oh) at 78.3°c kj determine the amount of heat energy (in kj) required to increase the temperature of 26.0 g of water from 370°c to 98 2°c kj. The equation that relates heat (q) (q) to specific heat (cp) (c p), mass (m) (m), and temperature change (Δt) (Δ t) is shown below. q = cp × m × Δt q = c p × m × Δ t. the heat that is either absorbed or released is measured in joules. the mass is measured in grams. the change in temperature is given by Δt = tf −ti Δ t = t f − t i.
Solved Please Help Determine The Amount Of Energy Require To get heat in joules: q = (25 g)x (334 j g) q = 8350 j. it's just as easy to express the heat in terms of calories: q = m·Δh f. q = (25 g)x (80 cal g) q = 2000 cal. answer: the amount of heat required to melt 25 grams of ice is 8,350 joules or 2,000 calories. note: heat of fusion should be a positive value. The amount of heat required to change 25 grams of water into steam is 56425 joules or 13500 calories. a related example illustrates how to calculate the energy when water changes from solid ice into steam . Determine whether you want to warm up the sample (give it some thermal energy) or cool it down (take some thermal energy away). insert the amount of energy supplied as a positive value. if you want to cool down the sample, insert the subtracted energy as a negative value. for example, say that we want to reduce the sample's thermal energy by. The fraction of molecules with energy equal to or greater than e a is given by the exponential term e−ea rt e − e a r t in the arrhenius equation: k = ae−ea rt (6.2.3.3.5) (6.2.3.3.5) k = a e − e a r t. k is the rate constant. e a is the activation energy. r is the gas constant.
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