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200.0 Joules of heat is required to raise the temperature of an object sample by 3.00C If the specific heat of the object is 01490 JgC what is the mass of the sample in kilograms?
Wiki User
∙ 10y ago
Use the equation for specific heat: energy = mass x (temperature difference) x (specific heat). Replace the numbers you know, and solve for mass. Since it seems that the specific heat is specified per gram, you'll initially get the mass per gram. Converting that to kilograms is quite easy.
Wiki User
∙ 10y ago
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Which could not be units for a vector quantity?
-- dollars -- weeks -- kilograms -- degrees (of temperature) -- pages -- watts -- decibels -- joules -- lumens
How many calories are required to increase the temperature of 13g of alcohol from 11 celsius to 23 celsius?
2.460 is the specific heat of ethyl alcohol in J/gC, so I will find joules and then convert to calories. q(joules) = mass*specific heat*change in temp. q = (13 g alcohol )(2.460 J/gC)(23 C - 11 C) = 383.76 joules (1 calorie/4.184 joules) = 92 calories ------------------
What is the quantity of heat in joules needed to raise the temperature of 40.0g of Al from 25 degrees Celsius to 50 degrees Celsius?
E = mass x specific heat x Δ°T Δ°T = new temperature - original temperature where Δ°T is equal to temperature change (Celsius in this case). The specific heat of Al is 0.900 J/g°C. Before we proceed to find the quantity of heat in joules, we must first find the temperature change. To calculate the temperature change, we must subtract the original temperature from the new temperature. Δ°T = 50°C - 25°C = 25°C In order to find the quantity of heat (joules), we must multiply mass, specific heat, and the temperature change (calculated above). E = 40.0g x 0.900 J/g°C x 25°C = 900 Joules or 9.0 x 102 Joules
How many joules of energy are required to raise the temperature of 20g of aluminum from 10 degrees C to 15 degrees C?
Heat energy Q = mass x specific heat capacity x temperature change. Q = m*c*delta T Q = Joules m = kg c (aluminum) = 895.8 J/kg delta T = degr.C temp. change Answer: Q = (20/1000) x 895.8 x 5 = 89.58 Joules (Specific heat capacity of aluminum is obtained by multiplying its specific heat of 0.214 with c of water which is 4186 J/kg = 0.214 x 4186 = 895.8 J/kg).
How many joules are absorbed by the water with a mass of 8 kg in order to raise the temperature from 20 degrees to 70 degrees?
q(joules) = mass * specific heat * change in temperature ( 8 kg = 8000 grams ) q = (8000 grams H2O)(4.180 J/gC)(70o C - 20o C) = 1.7 X 106 joules ============
How many kilojoules of energy are necessary to raise the temperature of 3 kilograms of cast iron from 30 degrees celsius to 120 degrees celsius?
I will use this formula. Some conversion will be required. ( I only know specific heat iron in J/gC ) q(Joules) = mass * specific heat * change in temperature Celsius 3 kilograms cast iron = 3000 grams q = (3000 g)(0.46 J/gC)(120 C - 30 C) = 124200 Joules (1 kilojoule/1000 joules) = 124.2 kilojoules of energy needed ===========================
What is the quantity of heat in joules or calories required to raise the temperature of 1 gram of a substance 1C.?
specific heat(; your welcome!
What is the quantity of heat in joules or calories required to raise the temperature of 1 gram of a substance 1C?
specific heat(; your welcome!
The specific heat of the material is?
specific heat content is calculated by the joules of energy required to change the temperature of one cubic centimeter of the material 1 degree Celsius.
Correct units to determine specific heat?
Specific heat is the heat required to raise the temperature of a unit mass by one degree. It is measured by joules.
How many joules are required for boiling 21.1g of water at 100C?
You need o know the initial temperature of water:Heat = specific heat x difference of temperature x mass of water
Which could not be units for a vector quantity?
-- dollars -- weeks -- kilograms -- degrees (of temperature) -- pages -- watts -- decibels -- joules -- lumens
How many calories are required to raise the temperature of 150 g sample of gold from 25 Celsius to 175 Celsius?
I will use this formula, the convert. q( in Joules ) = mass * specific heat Au * change in temp. q = nCT q = (150 grams)(0.129 J/gC)(175 C - 25 C) = 2902.5 Joules Now, 1 calorie = 4.184 Joules 2902.5 Joules (1 calorie/4.184 Joules) 694 calories required
How many calories are required to increase the temperature of 13g of alcohol from 11 celsius to 23 celsius?
2.460 is the specific heat of ethyl alcohol in J/gC, so I will find joules and then convert to calories. q(joules) = mass*specific heat*change in temp. q = (13 g alcohol )(2.460 J/gC)(23 C - 11 C) = 383.76 joules (1 calorie/4.184 joules) = 92 calories ------------------
Which would require a greater amount of heat water or iron?
To raise the temperature of both an equal amount, water would require more energy. In terms of the energy required to raise the temperature: iron = 0.45 joules / gram . kelvin water = 4.2 joules / gram . kelvin This is known as the specific heat capacity of a material
How do you find a mass of a substance dissolved in a solution given temperature and joules?
You can find the mass of a substance dissolved in a solution given temperature and joules using the relation q=mc(change in T). Where q is heat in joules, m is the mass, c is the specific heat capacity, and T is the temperature.
How many joules are required to heat 177G of Mercury from 18 C to 233 C?
Doesn't look like there's any phase change in this temperature range so you can use the heat flow equation; mass x specific heat x temperature change; where mass = m = .177 kg specific heat = C = 139 joules/kg-deg Temperature change = (Tf - Ti ) = 215 Q = .177 x 139 x 215 = 5289.6 joules I change mass to Kg so it would have same mass units as specific heat.
