If the specific heat of water is 1.0 calorie/gram°C, how many calories are required to raise 500 grams of water 10.0°C?
heat=mass*c*deltaT
= 500*1*10=5000 calories
poopoo
To calculate the calories required to raise the temperature of water, you can use the following formula:
Q = m * c * ΔT
Where:
Q = Heat energy in calories
m = Mass of water in grams
c = Specific heat capacity of water in calories/gram°C
ΔT = Change in temperature in °C
Given:
m = 500 grams
c = 1.0 calorie/gram°C
ΔT = 10.0°C
Substituting the values into the formula:
Q = 500 grams * 1.0 calorie/gram°C * 10.0°C
Q = 5000 calories
Therefore, 5000 calories are required to raise 500 grams of water by 10.0°C.
To find out how many calories are required to raise 500 grams of water 10.0°C, you need to use the formula:
Q = m * c * ΔT
where:
Q is the energy (in calories) required,
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in calories/gram°C), and
ΔT is the change in temperature (in °C).
In this case, m = 500 grams, c = 1.0 calorie/gram°C, and ΔT = 10.0°C. Plugging these values into the formula:
Q = 500 grams * 1.0 calorie/gram°C * 10.0°C
Q = 5000 calories
Therefore, 5000 calories are required to raise 500 grams of water 10.0°C.