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When two materials are rubbed together, it can cause a transfer of electrons between them, resulting in a build-up of static electricity. This can lead to various effects such as a spark discharge, attraction or repulsion of objects, or even a mild electric shock.

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1y ago

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How much heat is required to convert 75 g of ice from 0 C to liquid water at 90 C answer in cal?

Heat of fusion is absorbed Q = mLf = 75x 80 = 6000 cal just to melt the ice Heat is absorbed to change temp Q = mC(delta)T = 75 x 1 x (90 - 0) = 6750 cal Total heat = 6000 + 6750 = 12750 calories


How 1.987 Cal convert into joule?

1 calorie equals 4.18400 joules so multiply 1.987 by 4.184. 1.987 cal equals 8.313608 J.


What is specific heat of a substance if 1560 cal are required to raise the temperature of a 312g sample by 15 degrees C elsius?

q = m x C x ΔT q = amount of heat energy gained or lost by substance = 1560 calories m = mass of sample in grams = 312g C = heat capacity (calorie/g oC) =? ΔT = change in temperature = 15 oC Solve for C C = q/mΔT = 1560cal/(312g)(15 oC) = 0.33cal/g oC


How many calories of heat are needed to make glass rise 10 C?

It takes 1 calorie to raise 1 gram of water 1°C. Therefore, the specific heat of water is 1 cal/g°C.The specific heat of glass depends on it's composition. Plain/window glass is 0.2 cal/g°C; Crystal/plate glass is 0.12 cal/g°C; and Pyrex glass is 0.18 cal/g°C.To raise 1 gram of glass 10°C would then take between 1.2 and 2.0 calories.


The specific heat of a certain type of cooking oil is 1.75 cal(g and middot and degC). How much heat energy is needed to raise the temperature of 2.40 kg of this oil from 23 and degC to 191 and degC?

The change in temperature is ΔT = 191°C - 23°C = 168°C. The heat energy Q required is given by the formula Q = mcΔT, where m is the mass, c is the specific heat, and ΔT is the temperature change. Plugging in the values: Q = 2.4 kg * 1.75 cal/(g°C) * 168°C = 7056 cal = 7.056 kcal.