calculate the energy, in joules and calories
required to heat 25.0g of water form 12.5 deg. celcius to 25.7 deg. celcius i know the answer just need to see how to do it especially the calories
q = mass x specific heat water x delta T
q = 25.0g x 1 cal/g*C x (25.7-12.5) = ?
For joules, substitute 4.18 J/g*C for 1 cal/g*C
Well, I hope you're ready for a "heating" performance because it's time to calculate the energy required to heat that water!
To do this, we'll need to use the equation:
q = mcΔT
Where q is the energy required, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.
Let's start with joules. The specific heat capacity of water is approximately 4.18 J/g°C.
So, plugging in the values:
m = 25.0g
c = 4.18 J/g°C
ΔT = (25.7 - 12.5) = 13.2°C
q = (25.0g) * (4.18 J/g°C) * (13.2°C)
= 1,729.2 J
Now, let's convert this to calories. The conversion factor from joules to calories is 1 cal = 4.184 J.
For calories, we have:
q = 1,729.2 J / 4.184 J/cal
≈ 413.5 cal
So, the energy required to heat 25.0g of water from 12.5°C to 25.7°C is approximately 1,729.2 joules or 413.5 calories.
Now that we've warmed up our mathematical skills, we can turn up the heat on some jokes if you'd like!
To calculate the energy required to heat a substance, you can use the formula:
Q = mcΔT
Where:
Q is the energy (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in joules per gram per degree Celsius), and
ΔT is the change in temperature (in degrees Celsius).
First, let's find the energy in joules:
Given:
Mass of water (m) = 25.0g
Change in temperature (ΔT) = (25.7°C - 12.5°C) = 13.2°C
Specific heat capacity of water (c) = 4.18 J/g°C (this value may vary slightly depending on the source, but 4.18 is a commonly used approximation)
Now substitute the values into the formula:
Q = (25.0g) × (4.18 J/g°C) × (13.2°C)
Q = 1,729.6 J
Therefore, the energy required to heat 25.0g of water from 12.5°C to 25.7°C is 1,729.6 joules.
To convert joules to calories, you can use the conversion factor:
1 calorie = 4.184 joules
Now, let's convert the energy to calories:
Energy in calories = (1,729.6 J) / (4.184 J/cal)
Energy in calories ≈ 413.89 cal (rounded to two decimal places)
Therefore, the energy required to heat 25.0g of water from 12.5°C to 25.7°C is approximately 413.89 calories.
To calculate the energy required to heat water, you need to use the formula:
Q = m * C * ΔT
Where:
Q is the energy required (in Joules),
m is the mass of the water (in grams),
C is the specific heat capacity of water (4.18 J/g·°C),
ΔT is the change in temperature (in °C).
We can start by calculating the energy in joules:
1. Determine the mass (m) of the water: m = 25.0 g
2. Calculate the change in temperature (ΔT):
ΔT = final temperature - initial temperature
= 25.7°C - 12.5°C
= 13.2°C
3. Calculate the energy (Q) in joules using the formula:
Q = m * C * ΔT
= 25.0 g * 4.18 J/g·°C * 13.2°C
≈ 1,096.8 Joules
Therefore, the energy required to heat 25.0g of water from 12.5°C to 25.7°C is approximately 1,096.8 Joules.
To convert Joules to calories, note that 1 calorie (cal) is equal to 4.18 Joules:
1. Divide the energy in joules by the conversion factor:
Energy in calories = Energy in joules / Conversion factor (1 cal = 4.18 J)
= 1,096.8 J / 4.18
≈ 262.91 calories
Therefore, the energy required to heat 25.0g of water from 12.5°C to 25.7°C is approximately 262.91 calories.